Gibbs Quest: thermodynamics
Embark on a thrilling journey through thermodynamics, answering progressively tougher questions on Gibbs Free Energy to prove your mastery of spontaneous reactions and equilibrium.
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Topics of this game:
- What is Gibbs Free Energy used to predict?
- If a reaction has a negative value for ∆G, what does this indicate?
- Which of the following terms represents the change in disorder in a system?
- Which of these is a standard condition for temperature when calculating standard Gibbs Free Energy (∆G)?
- Which of the following factors is directly involved in the calculation of Gibbs Free Energy under non-standard conditions?
- If the equilibrium constant K is greater than 1, what can we say about ∆G°?
- If the reaction quotient Q is greater than the equilibrium constant K, what is the sign of ∆G?
- Which of the following equations is used to calculate ∆G at non-standard conditions?
- If the value of the equilibrium constant K for a reaction is very small (e.g., K = 10^(-5)), what can we infer about the value of ∆G°?
- At 298 K, if ∆G° = -50.0 kJ/mol and the reaction quotient Q = 0.1, what is the sign of ∆G?
- What happens to ∆G if the temperature of a reaction increases, and ∆H is positive while ∆S is negative?
- Given ∆G° = -30 kJ/mol and Q = 0.5 at 298 K, calculate ∆G using the equation, ∆G = ∆G° + RTlnQ.
- If a reaction has a positive ∆H, a positive ∆S, and occurs at a high temperature, what is the expected sign of ∆G?
- Calculate ∆G° for the following reaction at 298 K: N2(g) + 3H2(g) <-> 2NH3(g) Given: ∆H° = -92.4 kJ/mol ∆S° = -198.3 J/molK
- A chemical reaction at 298 K has the following parameters: ∆H° = -40.0 kJ/mol ∆S° = 150 J/molK Q = 0.25 Calculate the Gibbs Free Energy under these non-standard conditions.
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