by ftowne
Thermochemistry delves into the energetic changes that occur during chemical reactions and physical transformations. This quiz will challenge your understanding of concepts such as enthalpy, entropy, and Gibbs free energy. Sharpen your knowledge and see how well you grasp the principles that govern the energy dynamics in chemistry.
We recommend that you do not leave the page that you are taking this quiz in. Stay honest 🙂
Thermochemistry Quiz Questions Overview
1. What is the definition of enthalpy?
The total energy of a system
The heat content of a system at constant pressure
The randomness or disorder of a system
The energy required to start a reaction
2. Which of the following is a state function?
Work
Heat
Enthalpy
Power
3. What does the symbol ΔH represent in thermochemistry?
Change in entropy
Change in enthalpy
Change in internal energy
Change in temperature
4. Which law states that the total energy of an isolated system is constant?
First Law of Thermodynamics
Second Law of Thermodynamics
Third Law of Thermodynamics
Law of Conservation of Mass
5. What is the standard enthalpy change of formation?
The enthalpy change when one mole of a compound is formed from its elements in their standard states
The enthalpy change when one mole of a compound is decomposed into its elements
The enthalpy change when one mole of a substance is burned in oxygen
The enthalpy change when one mole of a substance dissolves in water
6. What is entropy a measure of?
The heat content of a system
The energy required to start a reaction
The randomness or disorder of a system
The total energy of a system
7. Which of the following reactions is exothermic?
Melting of ice
Evaporation of water
Combustion of methane
Photosynthesis
8. What does a negative ΔG (Gibbs free energy change) indicate about a reaction?
The reaction is non-spontaneous
The reaction is at equilibrium
The reaction is spontaneous
The reaction requires energy input
9. Which of the following is true for an endothermic reaction?
ΔH is negative
ΔH is positive
ΔS is negative
ΔS is positive
10. What is the unit of measurement for enthalpy change (ΔH)?
Joules (J)
Watts (W)
Kelvin (K)
Moles (mol)
11. Which principle states that the total enthalpy change of a reaction is the same, regardless of the number of steps?
Le Chatelier’s Principle
Hess’s Law
Boyle’s Law
Charles’s Law
12. What is the term for the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius?
Heat capacity
Specific heat capacity
Latent heat
Enthalpy
13. What is the significance of the standard state in thermochemistry?
It ensures all measurements are taken at 0 Kelvin
It provides a reference point for measuring thermodynamic properties
It indicates the most stable form of a substance at absolute zero
It is used to measure the heat content of a system
14. Which of the following is an example of a spontaneous process?
Ice melting at room temperature
Water freezing at room temperature
Iron rusting
Photosynthesis
15. What does the term ‘enthalpy of fusion’ refer to?
The enthalpy change when a substance melts
The enthalpy change when a substance vaporizes
The enthalpy change when a substance condenses
The enthalpy change when a substance freezes
16. What is the relationship between Gibbs free energy (ΔG), enthalpy (ΔH), and entropy (ΔS)?
ΔG = ΔH – TΔS
ΔG = ΔH + TΔS
ΔG = ΔH / TΔS
ΔG = ΔH * TΔS
17. Which of the following describes an exergonic reaction?
ΔG is positive
ΔG is negative
ΔH is positive
ΔS is negative
18. What is the heat capacity of a substance?
The amount of heat required to raise the temperature of one gram of the substance by one degree Celsius
The amount of heat required to raise the temperature of a given quantity of the substance by one degree Celsius
The amount of heat required to vaporize one mole of the substance
The amount of heat required to melt one mole of the substance
We recommend that you do not leave the page that you are taking this quiz in. Stay honest 🙂
