For a reaction carried out at

CHEMISTRY · Single correct · AP · Chemistry · Equilibrium · Equilibrium

Problem

298\,\text{K}

\Delta G^{\circ}

is reported to be

-35\,\text{kJ mol}^{-1}

. Which statement about the equilibrium constant

K

for this reaction is MOST accurate? (a)

K

is much less than 1 because the negative value of

\Delta G^{\circ}

makes

\ln K

negative. (b)

K

is approximately 1 since

\Delta G^{\circ}/(RT)\approx 0.01

298\,\text{K}

. (c)

K

is on the order of

10^{6}

; a large negative

\Delta G^{\circ}

means the equilibrium lies far toward products. (d)

K

is roughly

10^{14}

because using

\log

instead of

\ln

in the calculation gives a much larger value.