Specific Heat Capacity

Practice Questions

College Chemistry › Specific Heat Capacity

Questions

A $120.5\text{g}$ block of silver initially at $20.0^\circ \text{C}$ absorbs $678\text{J}$ of heat. If the specific heat capacity of silver is $0.240\text{J/g C}$ , in degrees Celsius, what is the final temperature of the block of silver?

How much heat is needed to raise the temperature of 10.0 g of water from 10.0 oC to 35.0 oC?

Specific heat capacity for water is $4.18\frac{\textrm{J}}{\textrm{g }^{\circ}\textrm{C}}$

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

Specific heat of water is $4.18\frac{\textrm{J}}{\textrm{g }^{\circ}\textrm{C}}$

Specific heat of lead is $0.128\frac{\textrm{J}}{\textrm{g }^{\circ}\textrm{C}}$

How much heat does it require to make a $216.7\text{g}$ block of lead initially at $27.8^\circ \text{C}$ go to $60.2^\circ \text{C}$ ? The specific heat capacity of lead is $0.160\frac{\text{J}}{\text{g}^{\circ}\text{C}}$ .

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?

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