Unit 3 test: Thermochemistry Honors Form B

Front

What is the formula to calculate the amount of energy absorbed or released during a temperature change?

Back

q = m * c * ΔT, where q is the heat energy (in Joules), m is the mass (in grams), c is the specific heat capacity (in J/g°C), and ΔT is the change in temperature (in °C).

Front

Define specific heat capacity.

Back

Specific heat capacity is the amount of heat required to raise the temperature of 1 gram of a substance by 1°C.

Front

What is the difference between an endothermic and exothermic process?

Back

An endothermic process absorbs heat from the surroundings, while an exothermic process releases heat to the surroundings.

Front

What happens to the temperature of a substance during a phase change?

Back

The temperature remains constant during a phase change, even though heat is being added or removed.

Front

How does heat flow between two objects?

Back

Heat flows from an object at a higher temperature to an object at a lower temperature until thermal equilibrium is reached.

Front

What is the significance of the average kinetic energy in relation to temperature?

Back

Temperature is a measure of the average kinetic energy of the particles in a substance.

Front

What is sublimation?

Back

Sublimation is the process in which a solid changes directly into a gas without passing through the liquid phase.

Front

How do you determine which material will have the largest temperature change when heated with the same amount of energy?

Back

The material with the lowest specific heat capacity will have the largest temperature change when heated with the same amount of energy.

Front

What is the specific heat capacity of water?

Back

The specific heat capacity of water is approximately 4.18 J/g°C.

Front

If 10,000 J of energy is added to a substance with a specific heat of 0.50 J/g°C and a mass of 100 g, what is the change in temperature?

Back

ΔT = q / (m * c) = 10,000 J / (100 g * 0.50 J/g°C) = 200°C.