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WorksheetsThermochemistry
Total questions: 20
Worksheet time: 17mins
Define work.
the flow of energy caused by a chemical reaction
the flow of energy caused by a temperature difference
the result of a force acting through a distance
the capacity to do work
Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings?
q = +, w = +
q = +, w = -
q = -, w = +
q = -, w = -
Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings?
q = -, w = -
q = +, w = -
q = +, w = +
q = -, w = +
Calculate the change in internal energy (ΔE) for a system that is giving off 60.0 kJ of heat and is performing 855 J of work on the surroundings.
60.0 x 10^2 kJ
-60.9 kJ
-59.1 kJ
59.1 kJ
If energy flows into a chemical system and out of the surroundings, what is the sign of ΔEsystem?
ΔEsystem < 0
ΔEsystem = 0
ΔEsystem > 0
If the internal energy of the products of a reaction is higher than the internal energy of the reactants, what is the sign of ΔE for the reaction?
ΔE < 0
ΔE = 0
ΔE > 0
In which direction does energy flow?
into the system from the surroundings
from the system into the surroundings
Heat capacity is ______.
the quantity of heat required to change a system's temperature by 1°C
the quantity of heat required to lower the temperature of 1 mole of a substance by 1°C
the quantity of heat required to raise the temperature of 1 gram of a substance by 1°F
the quantity of heat required to raise the temperature of 1 liter of a substance by 1°F
the quantity of heat required to raise the temperature of 1 gram of a substance by 1°C
What is specific heat capacity?
The quantity of heat required to raise the temperature of 1 gram of a substance by 1°C
The quantity of heat required to lower the temperature of a substance by 1°F
The quantity of heat required to raise the temperature of 1 mole of a substance by 1°F
The quantity of heat required to change a system's temperature by 1°C
the quantity of heat required to lower the temperature of 1 liter of a substance by 1°F
In the formula q=mCΔT, what does 'm' represent?
Mass (g)
Molarity (M)
Meters (m)
Moles (mol)
Which of the following equations correctly represents how to calculate the change in temperature (ΔT)?
Initial temperature minus final temperature
Initial temperature multiplied by final temperature
Final temperature multiplied by initial temperature
Final temperature minus initial temperature
Explain what happens to the potential energy of a rock as it falls off the side of a cliff.
The kinetic energy decreases as the potential energy increases.
The kinetic energy decreases as the potential energy decreases.
The potential energy decreases as the kinetic energy increases.
The potential energy decreases as the kinetic energy decreases.
Which of the following statements best describes the Conservation of Energy principle?
Energy can be created but not destroyed.
Energy can neither be created nor destroyed, but it can change forms.
Energy can be destroyed but not created.
Energy can be transferred to the environment only.
Heat always flows from cold objects to hot objects.
True
False
Which metal below would be the best conductor of energy? The Specific Heat values are in the table.
Iron
Copper
Titanium
Silver
