What is the difference between a A) spontaneous reaction, B) nonspontaneous reaction, and C) a reaction...
What is the difference between a A) spontaneous reaction, B) nonspontaneous reaction, and C)
a reaction at equilibrium in terms of free energy levels of the product and reactants? What is
the sign of ΔG for each of these reactions? Can reactions have different amounts of reactants
and products at equilibrium?
Homework Answers
A) Spontaneous reactions are those in which the products are more stable than the reactants. It means that the reaction will go in the forward direction. For a spontaneous reaction the value of ΔG is negative.
B) Non-spontaneous reaction are those in which the reactants are more stable than the products. It means that the reaction will go in the backward direction. For a non-spontaneous reaction the value of ΔG is positive.
C) At equilibrium the value of ΔG is zero because at equilibrium a cell does not work.
A reaction can have different amount of product and reactants at equilibrium. At equilibrium the rate of forward reaction should be equal to the rate of backward reaction.
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