Chapter 6 Chemical Thermodynamics

1. What is the measure of the disorder or randomness in a system?

Enthalpy

Second Law of Thermodynamics

Entropy

State function

Entropy is a measure of the disorder or randomness in a system. It quantifies the number of possible arrangements or microstates that a system can have. A system with high entropy is more disordered and has more possible arrangements, while a system with low entropy is more ordered and has fewer possible arrangements. The concept of entropy is a fundamental principle in thermodynamics and is closely related to the Second Law of Thermodynamics, which states that the entropy of an isolated system always increases over time.

Explanation

Entropy is a measure of the disorder or randomness in a system. It quantifies the number of possible arrangements or microstates that a system can have. A system with high entropy is more disordered and has more possible arrangements, while a system with low entropy is more ordered and has fewer possible arrangements. The concept of entropy is a fundamental principle in thermodynamics and is closely related to the Second Law of Thermodynamics, which states that the entropy of an isolated system always increases over time.

2. In section 6.3, a pot of water on the stove is boiling at a slow boil. What will happen to the temp. of the water if the stove burner is turned up higher, causing the water to boil more rapidly?

If the stove burner is turned up higher, causing the water to boil more rapidly, the temperature of the water will increase. This is because increasing the heat input will provide more energy to the water, causing the water molecules to move faster and increase in temperature.

Explanation

If the stove burner is turned up higher, causing the water to boil more rapidly, the temperature of the water will increase. This is because increasing the heat input will provide more energy to the water, causing the water molecules to move faster and increase in temperature.

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4. What quantity of heat energy is needed to raise the temperature of 1 pound (454g) of aluminum from 25.0 degree celcius to its melting point, 660. degree Celcius (Csp(Al) = 0.900 J/g.Celcius
In example 6.2

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Explanation

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5. In chemistry, all of the energy exchanged between a system and its surroundings may be placed into what two categories?

In chemistry, energy exchanged between a system and its surroundings can be categorized into two main categories: heat and work. Heat refers to the transfer of energy due to a temperature difference, while work refers to the transfer of energy due to a force acting through a distance. These two categories encompass all forms of energy exchange in a chemical system, whether it involves heat transfer or work done on or by the system.

Explanation

In chemistry, energy exchanged between a system and its surroundings can be categorized into two main categories: heat and work. Heat refers to the transfer of energy due to a temperature difference, while work refers to the transfer of energy due to a force acting through a distance. These two categories encompass all forms of energy exchange in a chemical system, whether it involves heat transfer or work done on or by the system.

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6. Internal energy is a property that is known as _______________________.

Internal energy is a property that is known as a state function. This means that it only depends on the initial and final states of a system, regardless of the path taken to reach those states. The value of internal energy is independent of the specific process or how the system got to its current state. This property is important in thermodynamics as it allows for the calculation of changes in energy without needing to know the exact details of the process.

Explanation

Internal energy is a property that is known as a state function. This means that it only depends on the initial and final states of a system, regardless of the path taken to reach those states. The value of internal energy is independent of the specific process or how the system got to its current state. This property is important in thermodynamics as it allows for the calculation of changes in energy without needing to know the exact details of the process.

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7. Arrange the following systems in order of increasing randomness or disorder.

1 mol liquid ammonia
1 mol gaseous ammonia
1 mol solid ammonia

The correct answer is arranging the systems in order of increasing randomness or disorder. In this case, the systems can be arranged as follows: 1 mol solid ammonia, 1 mol liquid ammonia, and 1 mol gaseous ammonia. This is because the solid state has the least randomness or disorder, followed by the liquid state, and finally the gaseous state which has the highest randomness or disorder.

Explanation

The correct answer is arranging the systems in order of increasing randomness or disorder. In this case, the systems can be arranged as follows: 1 mol solid ammonia, 1 mol liquid ammonia, and 1 mol gaseous ammonia. This is because the solid state has the least randomness or disorder, followed by the liquid state, and finally the gaseous state which has the highest randomness or disorder.

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9. In an Endothermic Reaction, the products are ususally colder than the reactants because the ________________________ has been absorbed.

In an endothermic reaction, the reactants absorb heat from the surroundings in order to form the products. This absorption of heat is an essential part of the reaction and is responsible for making the products colder than the reactants.

Explanation

In an endothermic reaction, the reactants absorb heat from the surroundings in order to form the products. This absorption of heat is an essential part of the reaction and is responsible for making the products colder than the reactants.

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