Energy and Changes of State Quiz

When you heat a system, the energy will be stored. In what form is the energy stored?

If temperature is a measure of the movement of particles, why does a cup of water at 30˚C store more energy than a spoonful of water at 30˚C?

How can we maintain the thermal energy in a warm object or prevent a cold object from gaining thermal energy?

Which of the following affect the amount of thermal energy stored in an object?

Which of the following is the definition of specific heat capacity?

Which of the following are correct?

[question number = 07.2] Use some of the following words to complete the definition.

Specific, cool, leftover, latent, power, energy, 1, 100, 1000, mixture, state

Which of the following equations represents the relationship between the change in thermal energy, the mass of an object, the specific heat capacity, and the change in temperature?

Calculate the change in energy of a 10kg iron block if its temperature increases by 20˚C and its specific heat capacity is 450 J/kg °C.

[question number = 01.3] We have a block of copper with a mass of 5 kg and a specific heat capacity of 385 J/kg °C. We increase the temperature of the copper by 15 ˚C. Calculate the change in thermal energy.

[question number = 07.4] Calculate the mass of a block of platinum when the change in thermal energy is 50 J, the specific heat capacity is 0.12 J/kg °C, and the change in temperature is 10 °C.

Specific latent heat is different depending on the state change. It takes more energy to evaporate 1kg of a substance than it does to melt 1kg of the same substance. Using this information, determine which of the following is correct.

Calculate the energy required to change 1 kg of water from a solid to a liquid at 0˚C. The specific latent heat of fusion/melting for water is 334 kJ/kg.

[question number = 07.1] Calculate the specific latent heat of vaporisation/evaporation for carbon dioxide using the following information. You have a 1.5kg sample of carbon dioxide that changed state from a liquid to a gas. The energy required to evaporate it was 856.62 J