Before moving on, answer these multiple choice questions to see if you understand the concepts in this lesson.
Which of the following would take the most energy to increase the temperature by 10°C?
- 3.50 kg of water
- 15.0 kg of water
- 3.50 kg of silver
- 15.0 kg of silver
The amount of energy to change a substance's temperature depends on both the mass and the specific heat capacity.
The amount of energy to change a substance's temperature depends on both the mass and the specific heat capacity.
The amount of energy to change a substance's temperature depends on both the mass and the specific heat capacity.
The amount of energy to change a substance's temperature depends on both the mass and the specific heat capacity.
How much energy is needed to change the temperature of a 0.875 kg piece of gold from 14.5°C to 35.0°C? (cgold = 129 J/kg°C)
- 5.59 x 103 J
- 3.96 x 103 J
- 2.31 x 103 J
- 1.64 x 103 J
Use \(\mathsf{ Q = mc \Delta T }\) to solve.
Use \(\mathsf{ Q = mc \Delta T }\) to solve.
Use \(\mathsf{ Q = mc \Delta T }\) to solve.
Use \(\mathsf{ Q = mc \Delta T }\) to solve.
It takes 3125 J of energy to change a 0.50 kg substance by 15.2°C. What is the substance?
- water
- gold
- lead
- iron
Use \(\mathsf{ Q = mc \Delta T }\) to solve for c to identify the substance.
Use \(\mathsf{ Q = mc \Delta T }\) to solve for c to identify the substance.
Use \(\mathsf{ Q = mc \Delta T }\) to solve for c to identify the substance.
Use \(\mathsf{ Q = mc \Delta T }\) to solve for c to identify the substance.
A 2.50 kg block of iron at 45.5°C is added to a 1.25 kg cup of water at 22.0°C. What is the final temperature?
- 10.9°C
- 16.2°C
- 25.9°C
- 38.5°C
Use \(\mathsf{ (mc \Delta T)_1 = -(mc \Delta T)_2 }\) to solve for the final temperature of the mixture.
Use \(\mathsf{ (mc \Delta T)_1 = -(mc \Delta T)_2 }\) to solve for the final temperature of the mixture.
Use \(\mathsf{ (mc \Delta T)_1 = -(mc \Delta T)_2 }\) to solve for the final temperature of the mixture.
Use \(\mathsf{ (mc \Delta T)_1 = -(mc \Delta T)_2 }\) to solve for the final temperature of the mixture.
Summary
Questions answered correctly:
Questions answered incorrectly:
