Chemistry

Problem

At 298 K, a reaction has

\Delta G^{\circ}=+1.5\,\text{kJ}\,\text{mol}^{-1}

. Which statement about its equilibrium constant

K

is most accurate? a)

K

is slightly greater than 1 b)

K

is much less than 1 c)

K

is slightly less than 1 d)

K

is approximately equal to 1

Intuitive explanation

The key is recognizing that $\Delta G°$ and $K$ are directly linked through the fundamental equation $\Delta G° = -RT \ln K$ . Since $\Delta G°$ is small and positive, $K$ will be close to 1—meaning the reaction slightly favors reactants over products, but not dramatically. Use the relationship to estimate whether $K$ is greater than, less than, or roughly equal to 1, rather than calculating an exact value.

Intuitive explanation

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