Take R = 8.314 J mol^-1 K^-1. A reaction has Delta G deg = +9.0 kJ mol^-1 at 300 K. Which statements are correct?

The equilibrium constant at 300 K lies between 0.01 and 0.1

If a mixture has Q = 1.0 x 10^-3, the net reaction goes forward

The equilibrium constant at 300 K lies between 0.01 and 0.1

If a mixture has Q = 1.0 x 10^-3, the net reaction goes forward

Delta G deg of the reaction changes as Q changes

JEE Main levelOne or more correct optionsDifficulty 2 of 3ce143

Take $R = 8.314 J mo l^{- 1} K^{- 1}$ . A reaction has $Δ G^{\circ} = + 9.0 kJ mo l^{- 1}$ at $300 K$ . Which statements are correct?

K = e^{- 9000/ (8.314 \times 300)} = e^{- 3.608} = 0.0271

, which lies between 0.01 and 0.1. A mixture with

Q = 1 0^{- 3} < K

reacts forward even though

Δ G^{\circ} > 0

, since

Δ G = RT ln (Q / K) < 0

Δ G^{\circ}

is fixed at a given temperature and is zero at equilibrium only if

K = 1

; at equilibrium it is

Δ G

that is zero.