Factors Affects Of Chemical Reaction

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Factors Affects Of Chemical Reaction - Quiz

Questions and Answers
  • 1. 

    Which three factors affect the rate of a chemical reaction?

    • A.

      Catalyst, Product Concentration, Container Volume

    • B.

      Temperature, Reactant Concentration, Pressure

    • C.

      Temperature, Reactant Concentration, Catalyst

    • D.

      Temperature, Product Concentration, Container Volume

    Correct Answer
    C. Temperature, Reactant Concentration, Catalyst
    Explanation
    The rate of a chemical reaction can be influenced by several factors. One of the factors is temperature, as an increase in temperature generally leads to an increase in the rate of reaction due to the higher kinetic energy of the molecules. Another factor is reactant concentration, as a higher concentration of reactants increases the likelihood of successful collisions between particles, leading to a faster reaction rate. Lastly, the presence of a catalyst can also affect the rate of reaction by lowering the activation energy required for the reaction to occur, thereby increasing the rate.

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  • 2. 

    In the reaction 2A + B --> 2C + D, the -[A] per time was found to be 5.0  .  What is the rate of change of B?

    • A.

      25 M/min

    • B.

      10 M/min

    • C.

      2.5 M/min

    • D.

      5.0 M/min

    Correct Answer
    C. 2.5 M/min
    Explanation
    The rate of change of B can be determined by comparing the coefficients of B in the balanced chemical equation. In this reaction, the coefficient of B is 1, while the coefficient of C is also 1. Since the reaction is 2A + B --> 2C + D, the rate of change of B is equal to half the rate of change of C. Therefore, if the rate of change of C is 5.0 M/min, the rate of change of B would be 2.5 M/min.

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  • 3. 

    Consider the reaction which ammonia is synthesized from nitrogen and hydrogen gases: How is the rate of formation of ammonia related to the rate of consumption of hydrogen?

    • A.

      The rate of formation of ammonia is two thirds the rate of consumption of hydrogen

    • B.

      The rate of formation of ammonia is half the rate of consumption of hydrogen

    • C.

      The rate of formation of ammonia is equal to the rate of consumption of hydrogen

    • D.

      The rate of formation of ammonia is 1/5 times the rate of consumption of hydrogen

    Correct Answer
    A. The rate of formation of ammonia is two thirds the rate of consumption of hydrogen
    Explanation
    The rate of formation of ammonia being two thirds the rate of consumption of hydrogen suggests that for every three moles of hydrogen consumed, two moles of ammonia are formed. This indicates that the reaction is not stoichiometrically balanced, and that there is an excess of hydrogen in the reaction. As a result, the rate of formation of ammonia is slower compared to the rate of consumption of hydrogen.

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  • 4. 

    Use the information below to determine the order of the reaction with respect to the concentration of A. A + B -->  P Trial     [A]            [B]        rate 1          0.273       0.763    2.83 2          0.273       1.526    2.83 3          0.819       0.763    25.47

    • A.

      3

    • B.

      4

    • C.

      2

    • D.

      1

    Correct Answer
    C. 2
    Explanation
    The order of the reaction with respect to the concentration of A can be determined by comparing the rates of reaction for different concentrations of A while keeping the concentration of B constant. In this case, the concentration of B is constant at 0.763. By comparing trials 1 and 2, where the concentration of A is the same but the concentration of B is different, we can see that the rate of reaction remains the same. This suggests that the concentration of A does not affect the rate of reaction, indicating that the order of the reaction with respect to A is 0. Therefore, the correct answer is 2.

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  • 5. 

    Activation energy is required to initiate

    • A.

      Endothermic reactions only.

    • B.

      Neither exothermic or endothermic reactions.

    • C.

      Both exothermic and endothermic reactions.

    • D.

      Exothermic reactions only.

    Correct Answer
    C. Both exothermic and endothermic reactions.
    Explanation
    Activation energy is the minimum amount of energy required to start a chemical reaction. It is needed for both exothermic and endothermic reactions because it helps break the existing bonds in the reactants and form new bonds in the products. This energy barrier must be overcome for the reaction to proceed, regardless of whether the reaction releases energy (exothermic) or absorbs energy (endothermic). Therefore, activation energy is required for both types of reactions.

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  • 6. 

    The difference between the potential energy of the products and the potential energy of the reactants is the

    • A.

      Heat of fusion

    • B.

      Heat of reaction

    • C.

      Free energy

    • D.

      Activation energy

    Correct Answer
    B. Heat of reaction
    Explanation
    The heat of reaction refers to the difference in potential energy between the products and the reactants in a chemical reaction. It represents the amount of heat energy released or absorbed during the reaction. This energy difference determines whether the reaction is exothermic (releasing heat) or endothermic (absorbing heat). Therefore, the given correct answer is "heat of reaction."

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  • 7. 

    Which condition will increase the rate of a chemical reaction?

    • A.

      Increased temperature and decreased concentration of reactants

    • B.

      Increased temperature and increased concentration of reactants

    • C.

      Decreased temperature and decreased concentration of reactants

    • D.

      Decreased temperature and increased concentration of reactants.

    Correct Answer
    B. Increased temperature and increased concentration of reactants
    Explanation
    Increasing the temperature of a chemical reaction provides more energy to the reactant molecules, causing them to move faster and collide more frequently. This leads to an increase in the rate of the reaction. Similarly, increasing the concentration of reactants means that there are more particles available to collide with each other, resulting in a higher rate of reaction. Therefore, both increasing the temperature and the concentration of reactants will increase the rate of a chemical reaction.

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  • 8. 

    Given the reaction:     2 SO2(g) + O2(g) --> 2 SO3(g)  The rate of the forward reaction increases by adding more SO2 because the

    • A.

      Number of molecular collisions will increase

    • B.

      Temperature will increase

    • C.

      Forward reaction is endothermic

    • D.

      Reaction will shift to the left

    Correct Answer
    A. Number of molecular collisions will increase
    Explanation
    By adding more SO2, the number of molecular collisions will increase. In a chemical reaction, the rate of reaction is directly proportional to the number of collisions between reactant molecules. By increasing the amount of SO2, there are more molecules available to collide with the other reactant, O2. This increases the likelihood of successful collisions, leading to a higher rate of the forward reaction.

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  • 9. 

    The decomposition of nitrogen dioxide to nitrogen and oxygen is second-order with a rate constant k = 12.5 M-1 s-1. What is the half-life for the reaction if [NO2]0 = 0.00260 M

    • A.

      30.8 sec

    • B.

      0.0800 sec

    • C.

      0.0554 sec

    • D.

      61.5

    Correct Answer
    A. 30.8 sec
    Explanation
    The half-life of a second-order reaction can be calculated using the formula t1/2 = 1 / (k * [A]0), where k is the rate constant and [A]0 is the initial concentration of the reactant. In this case, the rate constant is given as 12.5 M-1 s-1 and the initial concentration of NO2 is 0.00260 M. Plugging these values into the formula, we get t1/2 = 1 / (12.5 * 0.00260) = 30.8 seconds. Therefore, the half-life for the reaction is 30.8 seconds.

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  • 10. 

    Which of the following graphs is linear for A --> products

    • A.

      Ln[A] versus t if first-order in A

    • B.

      Ln[A] versus t if second-order in A

    • C.

       versus  if second-order A

    • D.

      1/[A] versus t if first-order in A

    Correct Answer
    A. Ln[A] versus t if first-order in A
    Explanation
    The correct answer is ln[A] versus t if first-order in A. This is because in a first-order reaction, the natural logarithm of the concentration of A decreases linearly with time. Therefore, plotting ln[A] versus t will result in a straight line, indicating a linear relationship between ln[A] and t.

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  • 11. 

    For the reaction A --> B, the activation energy is  = 125 kJ/mol and the heat of reaction, H = 50. kJ/mol. What is the  for the reverse reaction in kJ/mol?

    • A.

      125 kJ/mol

    • B.

      -75 kJ/mol

    • C.

      75 kJ/mol

    • D.

      -125 kJ/mol

    Correct Answer
    C. 75 kJ/mol
    Explanation
    The activation energy for the reverse reaction is the same as the activation energy for the forward reaction, which is 125 kJ/mol. The heat of reaction, H, is not relevant to determining the activation energy for the reverse reaction.

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  • 12. 

    Which of the following will lower the activation energy for a reaction? 

    • A.

      Adding a suitable catalyst

    • B.

      Increasing the concentrations of reactants

    • C.

      Raising the temperature of the reaction

    • D.

      All of these options will lower the activation energy for a reaction

    • E.

      There is no way to lower the activation energy of a reaction

    Correct Answer
    A. Adding a suitable catalyst
    Explanation
    Adding a suitable catalyst will lower the activation energy for a reaction. A catalyst is a substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy. It achieves this by lowering the energy barrier that the reactants must overcome to form products. Therefore, adding a suitable catalyst reduces the amount of energy needed for the reaction to occur, making it easier for the reaction to take place.

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  • 13. 

    Refer to the equation below, where two mechanisms are proposed for the reaction of nitrogen dioxide with carbon monoxide: NO2(g) + CO(g) --> CO2(g) + NO(g) Mechanism I: NO2(g) + CO(g) --> CO2(g) + NO(g) (one step) Mechanism II: NO2(g) + NO2(g) --> NO3(g) + NO(g) (slow) NO3(g) + CO(g) --> CO2(g) + NO2(g) (fast) What is the predicted rate law for Mechanism II?  

    • A.

      Rate=k[NO2]

    • B.

      Rate=k[NO2][CO]

    • C.

      Rate=k[NO2]^2[CO]

    • D.

      Rate=k[NO2]^2

    Correct Answer
    D. Rate=k[NO2]^2
    Explanation
    The predicted rate law for Mechanism II is rate=k[NO2]^2. This is because the slow step in the mechanism involves the reaction NO2(g) + NO2(g) --> NO3(g) + NO(g), which is second order with respect to NO2. Therefore, the overall rate law for the mechanism is rate=k[NO2]^2.

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  • 14. 

    A catalyst works by doing what?

    • A.

      By increasing the kinetic energy of the molocules

    • B.

      By reducing the activiation energy

    • C.

      By increasing the activation energy

    • D.

      By providing a large surface area

    Correct Answer
    B. By reducing the activiation energy
    Explanation
    Rate of reaction is the only general terms used.

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  • 15. 

    What factors can alter the rate of a reaction?

    • A.

      Temperature

    • B.

      Molocule size

    • C.

      X ray absorption

    • D.

      Absorptivity

    Correct Answer
    A. Temperature
    Explanation
    Temperature is a factor that can alter the rate of a reaction. Increasing the temperature generally increases the kinetic energy of the molecules, leading to more frequent and energetic collisions between reactant molecules. This results in a higher reaction rate as more successful collisions occur, increasing the likelihood of effective collisions and the formation of products. On the other hand, decreasing the temperature lowers the kinetic energy, reducing the frequency and energy of collisions, and thus decreasing the reaction rate. Therefore, temperature plays a crucial role in determining the rate of a reaction.

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  • 16. 

    What is the Delta H value for this reaction?

    • A.

      572 kJ mol-1

    • B.

      1370 kJ mol-1

    • C.

      -572 kJ mol -1

    • D.

      1942 kJ mol -1

    Correct Answer
    C. -572 kJ mol -1
    Explanation
    The correct answer is -572 kJ mol -1. This value represents the change in enthalpy for the reaction. A negative value indicates that the reaction is exothermic, meaning it releases heat to the surroundings. In this case, the reaction is releasing 572 kJ of heat per mole of reactant.

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  • 17. 

    Activation energy is required to initiate

    • A.

      Endothermic reactions only.

    • B.

      Neither exothermic or endothermic reactions.

    • C.

      Both exothermic and endothermic reactions.

    • D.

      Exothermic reactions only.

    Correct Answer
    C. Both exothermic and endothermic reactions.
    Explanation
    Activation energy is the minimum amount of energy required for a chemical reaction to occur. It acts as a barrier that must be overcome for the reaction to proceed. This energy is needed for both exothermic and endothermic reactions because regardless of whether the reaction releases or absorbs energy, an initial input of energy is necessary to break the existing bonds and form new ones. Therefore, activation energy is required for both types of reactions.

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  • 18. 

    When NH4NO3 is dissolved in water, the temperature of the water decreases.  When NaOH is dissolved in a separate water sample, the temperature of the water increases.  Based on these observations, it can be concluded that the dissolving of

    • A.

      Both salts are endothermic.

    • B.

      Both salts are exothermic.

    • C.

      NH4NO3 is exothermic and the dissolving of NaOH is endothermic.

    • D.

      NH4NO3 is endothermic and the dissolving of NaOH is exothermic.

    Correct Answer
    D. NH4NO3 is endothermic and the dissolving of NaOH is exothermic.
    Explanation
    Based on the given observations, when NH4NO3 is dissolved in water, the temperature of the water decreases, indicating that it absorbs heat from the surroundings. This is characteristic of an endothermic process. On the other hand, when NaOH is dissolved in water, the temperature of the water increases, indicating that it releases heat into the surroundings. This is characteristic of an exothermic process. Therefore, it can be concluded that the dissolving of NH4NO3 is endothermic and the dissolving of NaOH is exothermic.

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  • 19. 

    Given the reaction:     2 SO2(g) + O2(g) --> 2 SO3(g)  The rate of the forward reaction increases by adding more SO2 because the

    • A.

      Number of molecular collisions will increase

    • B.

      Temperature will increase

    • C.

      Forward reaction is endothermic

    • D.

      Reaction will shift to the left

    Correct Answer
    A. Number of molecular collisions will increase
    Explanation
    By adding more SO2 to the reaction, the number of molecular collisions will increase. This is because the rate of a chemical reaction is directly proportional to the number of collisions between reactant molecules. Increasing the concentration of SO2 increases the chances of collisions between SO2 and O2 molecules, leading to a higher rate of the forward reaction.

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  • 20. 

    A collision model can only happen when two molecules collide just right?

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    False. A collision model can happen even if two molecules do not collide "just right." In the collision model, molecules collide with each other and undergo reactions, but the success of the reaction does not solely depend on the collision being perfect. Factors like the energy and orientation of the collision also play a crucial role in determining whether a reaction will occur. Thus, a collision model can involve collisions that are not perfect or ideal.

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  • 21. 

    A reaction only takes when a molecule separates?

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    This statement is false. A reaction can occur even when a molecule does not separate. Reactions involve the rearrangement of atoms and the formation of new bonds, which can happen within a single molecule or between multiple molecules. Separation of molecules is not a requirement for a reaction to take place.

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  • 22. 

    Does the collision model only apply to when molecules collide?

    • A.

      Yes

    • B.

      No

    Correct Answer
    B. No
    Explanation
    The collision model does not only apply to when molecules collide. It also applies to the interaction between particles, such as atoms or ions, in a chemical reaction. The collision model states that for a reaction to occur, particles must collide with sufficient energy and proper orientation. Therefore, the model is not limited to molecules but encompasses all types of particles involved in chemical reactions.

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  • 23. 

    On this graph, which letter represents the activation energy? (hint: it isn't F)

    • A.

      A

    • B.

      B

    • C.

      C

    • D.

      D

    • E.

      E

    Correct Answer
    C. C
    Explanation
    The activation energy is the energy required for a chemical reaction to occur. In this graph, the letter "c" represents the activation energy because it is the highest point on the graph, indicating the energy barrier that needs to be overcome for the reaction to proceed. The other letters on the graph represent different stages or products of the reaction, but only "c" represents the activation energy.

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  • Current Version
  • Mar 22, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Nov 04, 2014
    Quiz Created by
    Ameier
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