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## Example Questions

### Example Question #4 : Solutions, States Of Matter, And Thermochemistry

A block of silver initially at absorbs of heat. If the specific heat capacity of silver is , in degrees Celsius, what is the final temperature of the block of silver?

**Possible Answers:**

**Correct answer:**

Recall the equation that gives the relationship between change in temperature and amount of heat:

,

where ,

,

, and

Since the question asks for the final temperature, re-arrange the equation to solve for .

Substitute in the given values to solve for the final temperature.

### Example Question #1 : Specific Heat Capacity

The specific heat capacity is defined as the amount of heat energy necessary to change a given amount of a substance by a certain temperature. Which of the following correctly expresses the units of specific heat capacity?

**Possible Answers:**

**Correct answer:**

For this question, we're given a definition for the specific heat capacity of a substance and we're asked to identify the correct units for this term.

We can also recall the equation that relates all of these terms.

Rearranging this expression to isolate the term for the specific heat capacity gives us the following.

Next, we can recall what units would be appropriate to use for each of the following terms in the above expression. The term represents heat energy added to or removed from the system, so this value would be in units of joules. Next, the term represents the mass of the substance, so grams can be used for this term. Finally, the term represents the change in temperature of the substance, so we can use the absolute temperature in kelvins here.

Putting all this together gives us the following.

### Example Question #6 : Solutions, States Of Matter, And Thermochemistry

How much heat is needed to raise the temperature of 10.0 g of water from 10.0 ^{o}C to 35.0 ^{o}C?

Specific heat capacity for water is

**Possible Answers:**

**Correct answer:**

Recall the relationship between heat and specific heat capacity

Plug in known values and solve for *Q*

### Example Question #8 : Solutions, States Of Matter, And Thermochemistry

An insulated container is filled with 50.0 g of water at 15.0 ^{o}C. 120.0 g of lead is heated to 100 ^{o}C and added to the insulated container. What is the final temperature of the system once it comes to equilibrium?

Specific heat of water is

Specific heat of lead is

**Possible Answers:**

**Correct answer:**

Since Pb starts at a higher temperature than the water, we know that energy (in the form of heat) will be transferred from Pb to water. Due to the law of conservation of energy, the exact same amount of energy lost by Pb must be gained by water.

Recall that

Combining the two equations, we have

Combine like terms then solve for final temperature

### Example Question #7 : Solutions, States Of Matter, And Thermochemistry

How much heat does it require to make a block of lead initially at go to ? The specific heat capacity of lead is .

**Possible Answers:**

**Correct answer:**

Recall the equation that gives the relationship between the change in temperature and the amount of heat:

, where

,

, and

Substitute in the given values to find how much heat is required to increase the temperature of the block of lead the specified amount.

Make sure to round the answer to three significant figures.

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