Energy Concepts in Thermochemistry Quiz
Test your understanding of energy concepts in thermochemistry with these questions on laws, enthalpy, entropy, and more!
#1
Which law of thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another?
Zeroth law
First law
Second law
Third law
#2
What is the SI unit of energy?
#3
Which term refers to the energy required to raise the temperature of one gram of a substance by one degree Celsius?
Enthalpy
Entropy
Specific heat
Gibbs free energy
#4
In an exothermic reaction, what happens to the enthalpy change (ΔH)?
It increases
It decreases
It remains constant
It depends on the reaction
#5
Which term describes the total energy content of a system?
Enthalpy
Entropy
Internal energy
Gibbs free energy
#6
What is the standard state for enthalpy of formation?
1 atm pressure and 0°C temperature
1 atm pressure and 25°C temperature
1 atm pressure and 100°C temperature
10 atm pressure and 0°C temperature
#7
Which of the following statements is true regarding an endothermic reaction?
It releases heat to the surroundings
It absorbs heat from the surroundings
It neither absorbs nor releases heat
It depends on the specific reaction conditions
#8
What does a negative value of Gibbs free energy (∆G) indicate for a reaction?
The reaction is at equilibrium
The reaction is non-spontaneous
The reaction is spontaneous
The reaction is reversible
#9
Which of the following statements about Hess's Law is true?
It states that the enthalpy change of a reaction depends only on the initial and final states of the reactants
It allows the calculation of the overall enthalpy change for a reaction by summing the enthalpy changes for each step of the reaction
It describes the relationship between temperature and the equilibrium constant of a reaction
It is only applicable to ideal gases
#10
Which law of thermodynamics defines absolute zero as the point where entropy is at a minimum?
Zeroth law
First law
Second law
Third law
#11
What is the relationship between the standard enthalpy change (∆H°) and the standard internal energy change (∆U°) for a reaction at constant pressure?
∆H° = ∆U°
∆H° = ∆U° + PV
∆H° = ∆U° + P∆V
∆H° = ∆U° + nRT
#12
Which quantity represents the maximum amount of useful work that can be obtained from a system at constant temperature and pressure?
Enthalpy
Entropy
Gibbs free energy
Internal energy
#13
Which of the following is NOT a state function?
Enthalpy
Entropy
Work
Internal energy
#14
What is the relationship between the standard enthalpy of reaction (∆H°) and the heat of reaction (∆H) at non-standard conditions?
∆H° = ∆H + ∆nRT
∆H° = ∆H + P∆V
∆H° = ∆H + RTln(Q)
∆H° = ∆H + nRTln(Q)
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