Justify the following statements. 1. Reactions with <0 always have an equilibrium constant greater than 1. 2. Many thermodynamically feasible reactions do not occur under ordinary conditions. 3. At low temperatures, enthalpy change dominates the expression and at high temperatures, it is the entropy which dominates the value of .

1. =-2.303RT . Thus, when ^ 1). 2. Under ordinary conditions, the average energy of the reactants may be less than threshold energy. They require some activation energy to initiate the reaction. 3. = -T . At low temperature, T is small. Hence, dominates. At high temperature, T is large, i.e. dominates the value of .

Justify the following statements. 1. Reactions with <0 always hav…

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Question

Justify the following statements.

Reactions with $\Delta\text{G}<0$ always have an equilibrium constant greater than 1.
Many thermodynamically feasible reactions do not occur under ordinary conditions.
At low temperatures, enthalpy change dominates the $\Delta\text{G}$ expression and at high temperatures, it is the entropy which dominates the value of $\Delta\text{G}.$

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Answer

$\Delta\text{G}=-2.303\text{RT}\log\text{K}.$ Thus, when $\Delta\text{G}^\circ<0,$ K > 1).
Under ordinary conditions, the average energy of the reactants may be less than threshold energy. They require some activation energy to initiate the reaction.
$\Delta\text{G}=\Delta\text{H}-\text{T}\Delta\text{S}.$ At low temperature, $\text{T}\Delta\text{S}$ is small. Hence, $\Delta\text{H}$ dominates. At high temperature, $\text{T}\Delta\text{S}$ is large, i.e. $\Delta\text{S}$ dominates the value of $\Delta\text{G}.$

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