Which of the following statements regarding Gibbs free energy is CORRECT? A:If a

Question

Which of the following statements regarding Gibbs free energy is CORRECT?

A:If a reaction has a large and negative standard free energy change (G°), product formation will be favored in actual conditions unless the ratio of products to reactants is high enough to drive the reaction in the reverse direction.

B:If a reaction has a large and negative standard free energy change (G°), product formation will be favored in actual conditions unless the ratio of products to reactants is high enough to drive the reaction in the reverse direction.

-An explanation would be great!

Explanation / Answer

A)

The statemet is correct since

dG = Gprod - Greactants

dG = dG - RT*ln(Q)

Q = [products]/[reactnats]

so, if products < reactants and dG < 0, expect spontenous reactions

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