### All AP Physics 2 Resources

## Example Questions

### Example Question #1 : Thermodynamics

of energy is applied to an aluminum rod of unknown mass. Its temperature goes from to . What is the mass of the rod?

**Possible Answers:**

There is not enough information to determine the rod's mass

**Correct answer:**

The relevant equation for this problem is called the specific heat capacity equation:

In this equation, is the total energy in Joules, is the mass in grams, is the specific heat of the substance in Joules over grams times Coulombs , and is the change in temperature in Kelvins or degrees Celsius; which one you use doesn't matter because it's the change you need.

To find the mass of the rod when given the energy, specific heat, and change in temperature, we can rearrange the equation to this:

Now, we can plug in our numbers and solve:

### Example Question #2 : Thermodynamics

Which of the following best defines the zeroth law of thermodynamics in variable form?

**Possible Answers:**

**Correct answer:**

The zeroth law of thermodynamics states that if an object X is in thermal equilibrium with object Y, and object Y also in thermal equilibrium with object Z, then object X must also be in thermal equilibrium with object Z.

refers to the first law of thermodynamics.

refers to the second law of thermodynamics.

is the enthalpy equation.

refers to entropy.

The best choice is:

### Example Question #3 : Thermodynamics

You have of water in a container above a burner. If of energy is put into the container (assume all of it goes into the water), and the specific heat of water is , how much did the water's temperature rise?

**Possible Answers:**

There's not enough information to determine the temperature change

**Correct answer:**

The equation for temperature change given applied heat is

.

is the amount of heat energy, is the mass, is the specific heat, and is the change in temperature. In this problem, we're given the energy, the mass, and the specific heat, so we need to solve the equation for .

Rearranging to find the change in temperature:

Now, we can plug in our numbers.

Therefore, the water changed by about degrees celsius given that amount of energy applied.

### Example Question #1 : Heat Transfer And Thermal Equilibrium

You have of an unknown metal. If, after adding of energy to it, its temperature raises by , what is the metal's specific heat?

**Possible Answers:**

There is not enough information to determine the specific heat of this metal

**Correct answer:**

To find the specific heat of an unknown material given temperature change, mass, and energy applied, we use the following equation:

Plug in known values and solve.

### Example Question #2 : Heat Transfer And Thermal Equilibrium

How much energy does it take to raise of water by ?

**Possible Answers:**

**Correct answer:**

The equation that is needed is:

Plug in known values and solve.

### Example Question #3 : Heat Transfer And Thermal Equilibrium

The heat capacity for any given material is defined as the amount of heat that must be added to that material in order to increase its temperature by . However, the heat capacity for any given material can be measured under different conditions, such as constant pressure or constant volume.

How would the heat capacity for a material at constant volume differ from the heat capacity for that same material at constant pressure?

**Possible Answers:**

The heat capacity at constant volume is equal to the heat capacity at constant pressure

There is no way to tell; the relative values of the constant volume and constant pressure heat capacities depends on the material under consideration

The heat capacity at constant volume is greater than the heat capacity at constant pressure

The heat capacity at constant pressure is greater than the heat capacity at constant volume

**Correct answer:**

The heat capacity at constant pressure is greater than the heat capacity at constant volume

In this question, we're presented with the definition of heat capacity. We're also told that the heat capacity for any given material can be measured at 1) constant volume, or 2) constant pressure. We're being asked to determine whether the constant volume heat capacity is greater than, less than, or equal to the constant pressure heat capacity for the same material.

First, let's revisit the definition of heat capacity. It is the amount of heat that must be added to a material to raise the temperature of that material by .

Next, let's consider what is happening as we add heat to a material at constant volume. When the volume of a material is held constant, that means that it is prevented from expanding as heat is added. Thus, all of the heat being added is resulting directly in an increase in the average kinetic energy of the particles that make up that material. In other words, all of the heat being added results in a temperature increase.

Let's now consider what happens when heat is added to a material at constant pressure. In this situation, the material is allowed to expand as heat is added to it (because volume is not being held constant). Therefore, when heat is added to the material, some of the heat will result in an increased temperature, but some of the heat will also result in an expansion of the material. The consequence of this is that in order to increase the temperature of the material by a given amount at constant pressure, it will require more heat energy than at constant volume.

Again, the main point of this is as follows:

- Constant volume - all of the added heat results in increased temperature
- Constant pressure - some of the added heat results in increased temperature and some of the added heat results in expansion

Since only a fraction of the heat being added at constant pressure will actually result in a temperature increase, we'll have to add more heat in order to increase its temperature by a given amount, when compared to constant volume conditions.

### Example Question #4 : Heat Transfer And Thermal Equilibrium

of ethanol is at a temperature of and of methanol is at a temperature of . If the two gases are in an isolated system together and allowed to transfer heat between each other, at which temperature will they reach thermal equilibrium?

**Possible Answers:**

**Correct answer:**

Since the two gases are in an isolated system, we know that the heat lost by one is equal to the heat gained by the other. Furthermore, we know that the two gases will be in thermal equilibrium when they have the same temperature, which will be some value in between their two initial values. Since methanol is at a higher temperature, we can say that it will loose heat and ethanol will gain that same amount of heat:

Substituting in expressions for each of these, we get:

Where the final temperature is equal for both gases:

Now we simply need to rearrange for the final temperature:

We have all of these values, so time to plug and chug:

### Example Question #5 : Heat Transfer And Thermal Equilibrium

Suppose that a copper bar long is raised from a temperature of to . If the coefficient of thermal expansion for copper is , what is the final length of the bar?

**Possible Answers:**

**Correct answer:**

To find out how much the bar will change in length, we'll need to use the equation for thermal expansion, which is as follows:

If we plug in the values that we know, we can solve for the change in length of the bar.

Now, we just need to add this value to the original length of the bar, and we will have our final answer.

### Example Question #6 : Heat Transfer And Thermal Equilibrium

Ana is holding onto an ice cube. Why does it melt in her hand?

**Possible Answers:**

Her hand took energy from the ice cube

The ice cube gave off energy to her hand

The heat from her hand warms it

The cold leaves the ice cube

All of these

**Correct answer:**

The heat from her hand warms it

According to the second law of thermodynamics, heat flows from hot to cold. Thus, the heat from her hand flows into the ice cube, causing it to melt.

### Example Question #7 : Heat Transfer And Thermal Equilibrium

An ideal heat engine uses the atmosphere as a low temperature reservoir and boiling water as a hot temperature reservoir. Water boils at . How much more efficient is the heat engine on a cold day () than when it is hot outside ()?

**Possible Answers:**

times more efficient

Not enough information.

times more efficient

times more efficient

Equally efficient

**Correct answer:**

times more efficient

The efficiency of an ideal heat engine is given by:

, where and stand for hot and cold respectively. To use this equation our temperatures must be in Kelvin. Here is the equation to convert from Celsius to Kelvin.

.

The denominator does not change if the temperature is hot or cold, so we need only consider the numerator. Let's compare both calculations:

Hot Day:

Cold Day:

Comparing these two efficiencies, we see that the cold day is roughly times as efficient.