Gibbs Free Energy Chemistry Q2 BM
Understanding Gibbs Free Energy
Test your knowledge of Gibbs Free Energy concepts with this engaging quiz! Explore essential definitions, equations, and the conditions for spontaneity in chemical reactions.
Whether you’re a chemistry student or just curious, this quiz will help reinforce your understanding of thermodynamics.
- 9 multiple-choice questions
- Learn about enthalpy, entropy, and free energy
- Assess your comprehension of spontaneous reactions
Gibbs Free Energy is ____.
The energy available to do work in chemical reactions
The energy available to do mechanical work
The degree of disorder in a chemical
The branch of physics that deals with the relationships between heat and other forms of energy
What is the formula for ∆G
�T- S∆H
T∆S- ∆H
�H-∆T∆S
�H-T∆S
What does ∆G stand for?
Temperature in system (K)
Entropy change measured in (kJ/K)
Change in free energy (kJ)
Enthalpy change measured in (kJ)
What does ∆H mean?
Enthalpy change measured in (kJ)
Entropy change measured in (kJ/K)
Temperature in system (K)
Change in free energy (kJ)
What does T mean?
Enthalpy change measured in (kJ)
Temperature in system (K)
Entropy change measured in (kJ/K)
Change in free energy (kJ)
What does ∆S mean?
Enthalpy change (kJ)
Entropy change (kJ/K)
Change in free energy (kJ)
Temperature in system (K)
When is the reaction spontaneous?
If ∆G < 0
If ∆G = 0
If ∆G > 0
Find ∆G for a reaction if: ∆H=-218 kJ and ∆S=-765 J/K at 32 Celsius. Is the reaction spontaneous?
15.4 kJ, spontaneous
15.4 kJ, non-spontaneous
15.4 K, spontaneous
15.4 K, non-spontaneous
For reaction CO(g) + H2O(g) → CO2(g) + H2(g) find ∆G if: ∆H = -41.2 kJ and ∆S = -135 J/K at 25 Celsius (298 K)
-0.97 kJ, non-spontaneous
0.97 kJ, spontaneous
-0.97 K, spontaneous
-0.97 kJ, spontaneous
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