Biology - Section 1.3 An Introduction To Metabolism Quiz

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  • 1/64 Questions

    Defined, a catabolic reaction is:

    • When cells build complex substances from simpler subunits
    • When cells build simpler substances from simpler subunits
    • Reactions that result in the synthesis of complex substances
    • Reactions that result in the breakdown of complex substances
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About This Quiz

SBI 4U1: BIOLOGY - CHAPTER 1: SECTION 1.3 AN INTRODUCTION TO METABOLISM QUIZ
This quiz was created by Ryan Flores based on the content within the Nelson Biology 12 textbook.
Quiz password: biology12
Please report any mistakes/discrepancies.

Biology - Section 1.3 An Introduction To Metabolism Quiz - Quiz

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  • 2. 

    Defined, an anabolic reaction is:

    • When cells build complex substances from simpler subunits

    • When cells build simpler substances from simpler subunits

    • Reactions that result in the synthesis of complex substances

    • Reactions that result in the breakdown of complex substances

    Correct Answer
    A. When cells build complex substances from simpler subunits
    Explanation
    Anabolic reactions refer to the process in which cells build complex substances from simpler subunits. This process involves the synthesis of larger molecules or structures from smaller building blocks. It is the opposite of catabolic reactions, which involve the breakdown of complex substances into simpler components. Anabolic reactions are essential for growth, repair, and maintenance of cells and tissues in the body. They require energy input and are often facilitated by enzymes.

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  • 3. 

    Defined, metabolism is the sum of:

    • All the anabolic processes occurring within a cell/organism

    • All the anabolic and catabolic processes occurring within a cell/organism

    • All the catabolic processes occurring within a cell/organism

    • All the anabolic and catabolic processes surrounding the cell/organism

    Correct Answer
    A. All the anabolic and catabolic processes occurring within a cell/organism
    Explanation
    Metabolism refers to the chemical processes that occur within a cell or organism to maintain life. Anabolic processes involve the building up of complex molecules from simpler ones, while catabolic processes involve the breaking down of complex molecules into simpler ones. The correct answer states that metabolism is the sum of all the anabolic and catabolic processes occurring within a cell/organism, which is accurate because both types of processes are essential for maintaining the overall balance and energy requirements of the cell/organism.

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  • 4. 

    All forms of energy can be classified as:

    • Kinetic energy

    • Potential energy

    • Kinetic or potential energy

    • Higher kinetic energy

    Correct Answer
    A. Kinetic or potential energy
    Explanation
    All forms of energy can be classified as either kinetic energy or potential energy. Kinetic energy refers to the energy possessed by an object due to its motion, while potential energy refers to the energy stored in an object based on its position or condition. Therefore, the correct answer is "Kinetic or potential energy" as it encompasses both forms of energy.

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  • 5. 

    Work is done when energy is transferred from one body or place to another. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Work is defined as the transfer of energy from one body or place to another. When energy is transferred, work is being done. Therefore, the statement "Work is done when energy is transferred from one body or place to another" is true.

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  • 6. 

    The First Law of Thermodynamics states:1. The total amount of energy in the universe is constant.2. Energy can be created and destroyed, but cannot be converted from one form to another.3. The entropy of the universe increases with any change that occurs.4. If an object or process gains an amount of energy, it does so at the expense of a loss in energy somewhere else in the universe.

    • 1 and 3

    • 1, 2 and 4

    • 1, 3 and 4

    • 1 and 4

    Correct Answer
    A. 1 and 4
    Explanation
    The First Law of Thermodynamics states that the total amount of energy in the universe is constant, which corresponds to option 1. Additionally, it states that if an object or process gains energy, it does so at the expense of a loss in energy somewhere else in the universe, which corresponds to option 4. Therefore, the correct answer is 1 and 4.

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  • 7. 

    A diver jumps off a diving tower. When will the diver have highest kinetic energy?

    • At the top of the diving tower

    • Just when the diver approaches the water

    • Just after the diver jumps off the diving tower

    • When the diver is in the water

    Correct Answer
    A. Just when the diver approaches the water
    Explanation
    The diver will have the highest kinetic energy just when they approach the water. This is because kinetic energy is directly proportional to the speed of an object. As the diver falls from the diving tower, their potential energy is converted into kinetic energy. The diver accelerates as they fall due to gravity, and their speed increases. Therefore, the diver will have the highest kinetic energy just before they hit the water, as they will be moving at their maximum speed at that point.

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  • 8. 

    Nature does provide energy in a readily usable form. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The statement is false because nature does not provide energy in a readily usable form. Energy from nature, such as sunlight or wind, needs to be converted or harnessed before it can be used by humans. For example, solar panels are used to convert sunlight into electricity, and wind turbines are used to convert wind energy into electrical energy. Therefore, energy from nature requires some form of technology or infrastructure to make it usable.

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  • 9. 

    Chemical potential energy is an important form of energy in living systems. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Chemical potential energy is indeed an important form of energy in living systems. It refers to the energy stored in chemical bonds within molecules. This energy is released during chemical reactions and is crucial for various biological processes such as metabolism and cellular respiration. Therefore, the statement "Chemical potential energy is an important form of energy in living systems" is true.

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  • 10. 

    The measure of the stability of a covalent bond is called:

    • Covalent energy

    • Bond energy

    • Kinetic energy

    • Potential energy

    Correct Answer
    A. Bond energy
    Explanation
    Bond energy refers to the measure of the stability of a covalent bond. It represents the amount of energy required to break a covalent bond and separate the bonded atoms. A higher bond energy indicates a stronger and more stable bond. It is an important concept in chemistry as it helps in understanding the strength and reactivity of different chemical bonds.

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  • 11. 

    Bond energy is measured in kilojoules (kJ), and is equal to the minimum energy required to break one of bonds between two types of atoms. It is also equal to the amount of energy released when a bond is formed.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Bond energy is a measure of the strength of a chemical bond. It is defined as the energy required to break a bond between two atoms or the energy released when a bond is formed. This energy is typically measured in kilojoules (kJ). Therefore, the statement that bond energy is measured in kilojoules and is equal to the minimum energy required to break a bond and the energy released when a bond is formed is true.

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  • 12. 

    The energy required to break a bond is not equivalent to the relative stability of the bond. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The energy required to break a bond is indeed equivalent to the relative stability of the bond. This means that a stronger bond requires more energy to break, indicating higher stability. Therefore, the correct answer is false.

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  • 13. 

    When reactant bonds break:

    • Energy is released

    • Energy is absorbed

    • Energy is released, and then absorbed back

    • Nothing happens to the energy level

    Correct Answer
    A. Energy is absorbed
    Explanation
    When reactant bonds break, energy is absorbed. This is because breaking bonds requires an input of energy. The energy is used to overcome the attractive forces between the atoms in the reactant molecules, allowing the bonds to break. This absorption of energy is an endothermic process, meaning it requires energy to occur. Once the bonds are broken, the reactant molecules can rearrange and form new bonds, releasing energy in an exothermic reaction. However, in the specific context of the question, it focuses on the breaking of bonds, which requires an absorption of energy.

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  • 14. 

    When product bonds form:

    • Energy is released

    • Energy is absorbed

    • Energy is released, and then absorbed back

    • Nothing happens to the energy level

    Correct Answer
    A. Energy is released
    Explanation
    When product bonds form, energy is released. This is because the formation of bonds involves the rearrangement of atoms and the formation of more stable chemical compounds. This process releases energy, which is often in the form of heat or light. The released energy is a result of the formation of stronger chemical bonds, which have lower potential energy than the reactant molecules. Therefore, the correct answer is that energy is released.

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  • 15. 

    What kind of diagram shows the potential energy that takes place during a chemical reaction?

    • Free body diagram

    • Kinetic energy diagram

    • Potential energy diagram

    • High potential energy diagram

    Correct Answer
    A. Potential energy diagram
    Explanation
    A potential energy diagram shows the potential energy changes that occur during a chemical reaction. It illustrates the energy levels of the reactants and products, as well as any energy barriers or intermediates involved in the reaction. This diagram helps to visualize the energy changes and understand the overall energy profile of the reaction.

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  • 16. 

    The amount of energy needed to strain and break the reactants' bond is equal to the difference between the potential energy level of the transition state and the potential energy of the reactants. This is the definition of which term?

    • Activation point

    • Kinetic energy

    • Transition state

    • Activation energy

    Correct Answer
    A. Activation energy
    Explanation
    The correct answer is "Activation energy." Activation energy is defined as the amount of energy required to strain and break the reactants' bond, which is equal to the difference between the potential energy level of the transition state and the potential energy of the reactants.

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  • 17. 

    Defined, transition state is:

    • A temporary condition in which the bonds within reactants are forming and bonds between products are breaking

    • A temporary condition in which the bonds within reactants are breaking and bonds between products are forming

    • A temporary condition in which the energy within reactants is disassociating

    • A temporary condition when nothing happens in the reaction

    Correct Answer
    A. A temporary condition in which the bonds within reactants are breaking and bonds between products are forming
    Explanation
    The correct answer is "a temporary condition in which the bonds within reactants are breaking and bonds between products are forming." This explanation accurately describes the concept of a transition state in a chemical reaction. During a chemical reaction, reactant molecules undergo a temporary state where the bonds within the reactants are breaking, and new bonds between the products are forming. This transition state is a crucial step in the overall reaction process.

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  • 18. 

    More energy is released during bond formation than during bond breaking if:

    • The bonds in products and the bonds in reactants are stable

    • The bonds in products are more stable than those in the reactants

    • The bonds in products are less stable than those in the reactants

    • The bonds in products and the bonds in reactants are not stable

    Correct Answer
    A. The bonds in products are more stable than those in the reactants
    Explanation
    When the bonds in the products are more stable than those in the reactants, it means that the products have a lower energy state than the reactants. This implies that more energy was released during bond formation than was required during bond breaking. This is consistent with the principle of energy conservation, where the energy released during bond formation is equal to the energy required during bond breaking. Therefore, the statement that the bonds in products are more stable than those in the reactants explains why more energy is released during bond formation.

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  • 19. 

    When a reaction results in a net energy output, it is called a/an:

    • Endothermic reaction

    • Exothermic reaction

    • Slow reaction

    • Fast reaction

    Correct Answer
    A. Exothermic reaction
    Explanation
    An exothermic reaction is a reaction that releases energy in the form of heat or light. This means that the products of the reaction have less energy than the reactants, resulting in a net energy output. In an exothermic reaction, energy is being released from the system into the surroundings, making it the correct answer for a reaction that results in a net energy output.

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  • 20. 

    The amount of energy absorbed in breaking reactants is greater than the energy released in the formation of product bonds. This results in a net absorption of energy. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In chemical reactions, breaking the bonds of reactants requires energy input, while forming the bonds of products releases energy. If the energy absorbed in breaking the reactant bonds is greater than the energy released in forming the product bonds, there is a net absorption of energy. This means that more energy is required for the reaction to occur than is released, resulting in a net absorption of energy. Therefore, the statement is true.

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  • 21. 

    When a reaction results in a net absorption of energy, it is called a/an:

    • Endothermic reaction

    • Exothermic reaction

    • Slow reaction

    • Fast reaction

    Correct Answer
    A. Endothermic reaction
    Explanation
    An endothermic reaction is a type of reaction that results in a net absorption of energy. In this type of reaction, the products have higher energy than the reactants, and energy is taken in from the surroundings. This means that the reaction requires an input of energy to proceed.

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  • 22. 

    The overall change in energy that occurs in a chemical reaction is called:

    • Entropy of reaction

    • Transition state

    • Enthalpy of reaction

    • None of the above

    Correct Answer
    A. Enthalpy of reaction
    Explanation
    Enthalpy of reaction refers to the overall change in energy that occurs in a chemical reaction. It is a measure of the heat energy released or absorbed during a reaction. The enthalpy change can be positive (endothermic) if energy is absorbed, or negative (exothermic) if energy is released. This energy change is important in determining the feasibility and direction of a chemical reaction. Entropy of reaction refers to the change in disorder or randomness, while transition state refers to the high-energy intermediate state during a reaction. Therefore, the correct answer is Enthalpy of reaction.

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  • 23. 

    A value of delta H is positive for exothermic reactions, and negative for endothermic reactions. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The statement is false. A positive value of delta H indicates an endothermic reaction, where heat is absorbed from the surroundings. Conversely, a negative value of delta H indicates an exothermic reaction, where heat is released to the surroundings.

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  • 24. 

    In an exothermic reaction, the chemical potential energy is lower in the products than in the reactants. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In an exothermic reaction, the chemical potential energy is lower in the products than in the reactants. This is because exothermic reactions release energy in the form of heat or light, resulting in a decrease in the overall potential energy of the system. The reactants have higher potential energy, which is converted into other forms of energy during the reaction, causing the products to have lower potential energy than the reactants. Therefore, the statement is true.

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  • 25. 

    In an endothermic reaction, the chemical potential energy in the reactants is lower than in the products. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In an endothermic reaction, the reactants absorb energy from the surroundings, resulting in an increase in the chemical potential energy of the products. This means that the chemical potential energy in the reactants is indeed lower than in the products, making the statement true.

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  • 26. 

    What is the most common form of energy absorbed and released by chemical reactions in living things?

    • Light energy

    • Sound energy

    • Thermal energy

    • Light and thermal energy

    Correct Answer
    A. Thermal energy
    Explanation
    Chemical reactions in living things typically involve the breaking and forming of chemical bonds, which results in the absorption and release of energy. The most common form of energy involved in these reactions is thermal energy. This is because chemical reactions often result in changes in temperature, as energy is either absorbed or released in the form of heat. Therefore, thermal energy is the primary form of energy absorbed and released by chemical reactions in living things.

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  • 27. 

    Defined, entropy is:

    • The amount of heat released by a chemical reaction

    • A measure of the colour intensity of a chemical reaction

    • A measure of the randomness or disorder in energy or in a collection of objects

    • A measure of the randomness or disorder of particles in a collection of object

    Correct Answer
    A. A measure of the randomness or disorder in energy or in a collection of objects
    Explanation
    Entropy is a measure of the randomness or disorder in energy or in a collection of objects. It quantifies the level of chaos or randomness within a system. In thermodynamics, entropy is used to describe the distribution of energy within a system and how it tends to spread out over time. It is a fundamental concept in understanding the behavior of physical and chemical systems.

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  • 28. 

    When entropy increases, disorder increases. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    When entropy increases, it means that the system becomes more disordered. This is because entropy is a measure of the randomness or disorder in a system. Therefore, as entropy increases, the level of disorder in the system also increases.

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  • 29. 

    In chemical reactions, entropy increases when:1. Liquid reactants become gaseous products2. Solutes move from an area of high concentration to an area of low concentration until they are uniformly distributed in the volume3. Complex molecules react to form simpler molecules4. Fewer moles of reactant molecules form a greater number of moles of product molecules5. Solid reactants become liquid or gaseous products

    • 1 and 3

    • 1, 2, 4 and 5

    • 1, 2, 3, 4 and 5

    • 1, 2, 3 and 4

    Correct Answer
    A. 1, 2, 3, 4 and 5
    Explanation
    Entropy is a measure of the disorder or randomness in a system. In chemical reactions, entropy increases when there is an increase in the number of energetically equivalent ways that the particles can be arranged.

    1. When liquid reactants become gaseous products, there is an increase in the number of particles and the freedom of movement, leading to an increase in entropy.
    2. When solutes move from an area of high concentration to an area of low concentration until they are uniformly distributed, the system becomes more randomly arranged, increasing entropy.
    3. Complex molecules reacting to form simpler molecules leads to an increase in the number of particles and possible arrangements, increasing entropy.
    4. If fewer moles of reactant molecules form a greater number of moles of product molecules, there is an increase in the number of particles and possible arrangements, increasing entropy.
    5. When solid reactants become liquid or gaseous products, there is an increase in the freedom of movement and the number of particles, leading to an increase in entropy.

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  • 30. 

    What are the two factors that need to be taken into consideration when determining whether a given chemical or physical change will occur spontaneously?

    • Energy and reaction rate

    • Energy and concentration

    • Energy and mass

    • Energy and entropy

    Correct Answer
    A. Energy and entropy
    Explanation
    When determining whether a given chemical or physical change will occur spontaneously, two factors that need to be taken into consideration are energy and entropy. Energy refers to the amount of energy available or required for the change to occur. If the change requires energy input, it is less likely to occur spontaneously. On the other hand, if the change releases energy, it is more likely to occur spontaneously. Entropy, on the other hand, refers to the level of disorder or randomness in a system. Spontaneous changes tend to increase the overall entropy of a system. Therefore, both energy and entropy play crucial roles in determining the spontaneity of a chemical or physical change.

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  • 31. 

    Josiah Willard Gibbs discovered a relationship between what?

    • Energy change and temperature of a reaction

    • Energy change, entropy change, and temperature of a reaction

    • Energy change and entropy change

    • Entropy change and temperature of a reaction

    Correct Answer
    A. Energy change, entropy change, and temperature of a reaction
    Explanation
    Josiah Willard Gibbs discovered a relationship between energy change, entropy change, and temperature of a reaction. This means that these three factors are interconnected and influence each other in a chemical reaction. Gibbs' work on thermodynamics laid the foundation for understanding the relationship between energy, entropy, and temperature and their role in determining the spontaneity and direction of chemical reactions.

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  • 32. 

    Gibbs free energy is defined as energy that can do useful work. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Gibbs free energy is a thermodynamic potential that measures the maximum reversible work that can be performed by a system at constant temperature and pressure. It takes into account both the system's internal energy and the entropy change. Therefore, Gibbs free energy is indeed defined as energy that can do useful work, making the answer "True" correct.

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  • 33. 

    Changes are spontaneous when delta G is:

    • Positive

    • Negative

    • Decimal

    • A really large number

    Correct Answer
    A. Negative
    Explanation
    When delta G is negative, it indicates that the reaction is spontaneous and will proceed in the forward direction without the need for external energy input. This is because a negative delta G means that the products have a lower free energy than the reactants, resulting in a release of energy. Therefore, changes are spontaneous when delta G is negative.

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  • 34. 

    A reaction that is spontaneous in one direction is also spontaneous in the reverse direction. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    A reaction that is spontaneous in one direction is not necessarily spontaneous in the reverse direction. The spontaneity of a reaction depends on the difference in free energy between the reactants and products. If the forward reaction has a negative change in free energy, indicating spontaneity, the reverse reaction would have a positive change in free energy and would not be spontaneous. Therefore, the statement is false.

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  • 35. 

    Generally, when energy is changed from one form to another, some of it is lost as heat. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    When energy is changed from one form to another, some of it is lost as heat. This is due to the inefficiencies in the conversion process. Energy transformations are never 100% efficient, and a portion of the energy is always dissipated as heat. This principle is known as the law of conservation of energy, which states that energy cannot be created or destroyed, only transferred or transformed. Therefore, it is true that when energy is changed from one form to another, some of it is lost as heat.

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  • 36. 

    The Second Law of Thermodynamics states:

    • The enthalpy of the universe increases with any change that occurs

    • The enthalpy of the universe decreases with any change that occurs

    • The entropy of the universe decreases with any change that occurs

    • The entropy of the universe increases with any change that occurs

    Correct Answer
    A. The entropy of the universe increases with any change that occurs
    Explanation
    The Second Law of Thermodynamics states that the entropy of the universe increases with any change that occurs. Entropy is a measure of the disorder or randomness in a system. According to this law, any spontaneous process or change in a system will always result in an overall increase in the entropy of the universe. This means that over time, the universe tends to become more disordered. This law is based on the observation that natural processes are irreversible and tend to move towards a state of greater randomness.

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  • 37. 

    Living things build up their bodies and the world around them. They do this at the expense of the entropy of the universe as a whole. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Living things are able to build up their bodies and the world around them by using energy from their surroundings. This process involves organizing and structuring matter, which decreases the entropy (disorder) in their immediate environment. However, this decrease in entropy is offset by an increase in entropy elsewhere in the universe, maintaining the overall balance. Therefore, it is true that living things build up their bodies and the world around them at the expense of the entropy of the universe as a whole.

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  • 38. 

    Living organisms obey the Second Law of Thermodynamics. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Living organisms obey the Second Law of Thermodynamics because this law states that the entropy of a closed system, such as an organism, tends to increase over time. Entropy refers to the measure of disorder or randomness in a system. Living organisms consume energy and release waste products, which increases the overall entropy of the system. Therefore, it is true that living organisms follow the Second Law of Thermodynamics.

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  • 39. 

    Which law predicts the the universe will experience a final "heat death" in which all particules and energy move randomly about, unable to do useful work?

    • The First Law of Thermodynamics

    • The Second Law of Thermodynamics

    • The Third Law of Thermodynamics

    • A and B

    Correct Answer
    A. The Second Law of Thermodynamics
    Explanation
    The second law of thermodynamics predicts the "heat death" of the universe, where all particles and energy will eventually reach a state of maximum entropy and randomness. This law states that in any natural process, the total entropy of a closed system will always increase or remain constant, but it will never decrease. As the universe continues to expand and disperse, the available energy for useful work will be depleted, resulting in a state of equilibrium where no further work can be done.

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  • 40. 

    All the energy that every existed on Earth will disappear when it experiences a "heat death". True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    False. The statement is incorrect. According to the concept of "heat death," it is not that all energy will disappear, but rather that the universe will reach a state of maximum entropy where no more useful energy can be extracted. Energy will still exist but will be evenly distributed and unavailable for any meaningful work.

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  • 41. 

    The terms endothermic and exothermic are used to describe the change in total energy that takes place in a chemical reaction. The energy can now be described in terms of a change in Gibb's free energy as:

    • Exertonic and endertonic reactions

    • Exersonic and endersonic reactions

    • Exerdonic and enderdonic reactions

    • Exergonic and endergonic reactions

    Correct Answer
    A. Exergonic and endergonic reactions
    Explanation
    Exergonic and endergonic reactions are terms used to describe the change in total energy that occurs during a chemical reaction. Exergonic reactions release energy, usually in the form of heat, and have a negative change in Gibb's free energy. These reactions are spontaneous and do not require an input of energy. On the other hand, endergonic reactions require an input of energy and have a positive change in Gibb's free energy. These reactions are non-spontaneous and do not occur without an external source of energy.

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  • 42. 

    In an exergonic reaction:1. The reaction is spontaneous and is accompanied by a decrease in Gibb's free energy (delta G is negative)2. The reaction is not spontaneous and is accompanied by an increase in Gibb's free energy (delta G is positive)3. The value of delta G provides a measure of the amount of free energy released by the reaction4. The value of delta G provides a measure of the amount of free energy needed to drive the reaction

    • 1 and 2

    • 1 and 3

    • 3 and 4

    • 2 and 4

    Correct Answer
    A. 1 and 3
    Explanation
    In an exergonic reaction, the reaction is spontaneous and is accompanied by a decrease in Gibb's free energy (delta G is negative). Additionally, the value of delta G provides a measure of the amount of free energy released by the reaction. Therefore, the correct answers are 1 and 3.

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  • 43. 

    The reactions of metabolism are enzyme catalyzed and are all reversible. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    The statement is true because the reactions of metabolism, which involve the breakdown and synthesis of molecules, are catalyzed by enzymes. Enzymes speed up the reactions by lowering the activation energy required. Additionally, these reactions are reversible, meaning they can proceed in both the forward and backward directions depending on the conditions and concentrations of reactants and products. This allows for the dynamic regulation and balance of metabolic pathways in response to the needs of the organism.

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  • 44. 

    When a reversible reaction reaches equilibrium:

    • Its delta G value is zero

    • Its free energy content is zero

    • Its delta H is zero

    • A and B

    Correct Answer
    A. A and B
    Explanation
    When a reversible reaction reaches equilibrium, both the delta G value and the free energy content are zero. Delta G represents the change in Gibbs free energy, which is a measure of the spontaneity of a reaction. At equilibrium, the forward and reverse reactions occur at the same rate, and there is no net change in free energy. Therefore, both statements A and B are correct. Delta H, on the other hand, represents the change in enthalpy, which is not necessarily zero at equilibrium.

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  • 45. 

    A cell whose reversible reactions have reached equilibrium is a living cell. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The statement is false because a cell whose reversible reactions have reached equilibrium is not necessarily a living cell. Reversible reactions reaching equilibrium can occur in both living and non-living systems. Living cells are characterized by various processes and functions, such as metabolism, growth, and reproduction, which go beyond the concept of equilibrium in chemical reactions.

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  • 46. 

    Most of the reactions of metabolism are a series of chain reactions in which the product of one reaction is the reactant of another reaction. What happens to the final product of the chain?

    • It is stored within the cell

    • It is released into the external environment

    • It is used in another chain reaction

    • A and C

    Correct Answer
    A. It is released into the external environment
    Explanation
    The final product of the chain reaction is released into the external environment. This is because most reactions of metabolism are part of a larger process that involves multiple reactions. The product of one reaction becomes the reactant for the next reaction in the chain. Eventually, the final product is formed and it is released from the cell into the external environment. This allows the cell to eliminate waste products and maintain homeostasis.

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  • 47. 

    Adenosine triphosphate is commonly abbreviated as:

    • ANP

    • ATP

    • ADTP

    • ADP

    Correct Answer
    A. ATP
    Explanation
    Adenosine triphosphate is commonly abbreviated as ATP. ATP is a molecule that serves as the primary energy currency of the cell. It is involved in various cellular processes, including muscle contraction, nerve impulse transmission, and chemical synthesis. The abbreviation ATP is widely recognized and used in scientific literature and research.

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  • 48. 

    Adenosine triphosphate is the secondary source of free energy in living cells. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Adenosine triphosphate (ATP) is actually the primary source of free energy in living cells, not the secondary source. ATP is a molecule that carries and transfers energy within cells, providing the necessary energy for various cellular processes. It is produced through cellular respiration and is used as a fuel for metabolic reactions. Therefore, the correct answer is false.

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  • 49. 

    Adenosine triphosphate includes:

    • The purine nitrogenous base adenine attached to the five-carbon sugar ribose

    • Three phosphate groups

    • All of the above

    • None of the above

    Correct Answer
    A. All of the above
    Explanation
    Adenosine triphosphate (ATP) is a molecule that serves as the primary energy source for cellular processes. It consists of a purine nitrogenous base called adenine, which is attached to a five-carbon sugar called ribose. Additionally, ATP contains three phosphate groups. Therefore, the correct answer is "All of the above" as all the mentioned components are included in adenosine triphosphate.

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  • Dec 05, 2023
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  • Feb 21, 2010
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