Thermochemistry Test Question Preview (ID: 19263)


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Endothermic reactions will always drop in temperature
a) True
b) False
c)
d)

A reaction starts with less energy than what it ends with.
a) True
b) False
c)
d)

In an exothermic reaction the system gains energy in the form of heat
a) True
b) False
c)
d)

Endothermic reactions absorb energy from the surroundings
a) True
b) False
c)
d)

The change in temperature is a chemical property.
a) True
b) False
c)
d)

Energy is not given off to the environment
a) True
b) False
c)
d)

Which of the following is not a type of energy?
a) acidic
b) potential
c) chemical
d) kinetic

What is chemical energy?
a) potential energy stored in chemical bonds
b) energy from fire and explosions
c) energy used when turning on a metal burner
d) energy used by a roller coaster going down hill

What is heat?
a) the amount of thermal energy in something
b) how warm or cold something is
c) what our bodies give off to other people
d) measured in degrees Celsius

What happens to energy when things happen?
a) energy is transferred or conserved
b) sometimes we waste our energy
c) it goes away
d) when things happen we “use up our energy”

Which of the following is not a way energy is transferred?
a) concentration
b) conduction
c) convection
d) radiation

What sign does ∆H have in exothermic reactions?
a) negative
b) positive
c) neutral
d) none of these

What is the definition of enthalpy?
a) The quantity of heat required to raise the temperature of a sample of a substance one degree Celsius
b) Energy that transfers from one object to another because of a temperature difference between them
c) Change in heat content for a reaction at constant pressure
d) The unavailability of a system’s thermal energy to do work

Considering the following equation, how much energy would be released if 50.0g of water were reacted?2NH3 + 4H2O 2NO2 + 7H2 ∆H= -142.5 kJ
a) -99.0 kJ
b) -6.85 kJ
c) + 99.0 kJ
d) +6.85 kJ

Consider the following equation, how much energy would be released if 10.0g of C2H5OH were burned?C2H5OH + 3O2 2CO2 + 3H2O ∆H= -1234.7 kJ
a) -290 kJ
b) +268.4 kJ
c) + 290 kJ
d) -268.4 kJ

A 50-gram piece of silver is dropped into a container of water. As it cools, the silver gives off 200 calories of heat. What is the silver’s temperature change? (The specific heat capacity of silver is 0.056 cal/g°C).
a) 560 °C
b) 71.4 °C
c) 4.5 °C
d) 5.6 x 10-6 °C

A 20-gram piece of copper is dropped into a container of water. As it cools, the water changes from 40 °C to 60 °C. How much heat did the copper give off? (The specific heat capacity of copper is 0.092 cal/g°C).
a) 184 calories
b) 36.8 calories
c) 4,347.8 calories
d) 54.35 calories

A piece of sugar free gum is burned in a bomb calorimeter containing 500 g of water. The temperature of the water increases from 25 ºC to 35 ºC. How many calories did the sugar free gum have?
a) 5000 calories
b) 5 calories
c) 470 calories
d) 30,000 calories

A piece of sugar free gum is burned in a bomb calorimeter containing 500 g of water. The temperature of the water increases from 25 ºC to 35 ºC. How many Calories did the sugar free gum have?
a) 5000 calories
b) 5 calories
c) 470 calories
d) 30,000 calories

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