The equilibrium constant Kp for a homogeneous gaseous reaction is 10-8. The standard Gibbs free energy change Δ G ominus for the reaction (using R=2 cal -1 mol -1 ) is

Question

The equilibrium constant Kp for a homogeneous gaseous reaction is 10-8. The standard Gibbs free energy change Δ G ominus for the reaction (using R=2 cal -1 mol -1 ) is (A) 10.98 kcal (B) -1.8 kcal (C) -4.1454 kcal (D) +4.1454 kcal

Tardigrade Admin · Accepted Answer

Δ G ominus=-2.303 R T log K =-2.303 × 2 × 298 log 10-8 =-2.303 × 2 × 298 ×-8 cal =10980 cal =10.98 kcal

Q. The equilibrium constant $K_{p}$ for a homogeneous gaseous reaction is $1 0^{- 8}$ . The standard Gibbs free energy change $Δ G^{⊖}$ for the reaction (using $R = 2 c a l^{- 1} m o l^{- 1}$ ) is

$10.98 k c a l$

$- 1.8 k c a l$

$- 4.1454 k c a l$

$+ 4.1454 k c a l$

$Δ G^{⊖} = - 2.303 RT lo g K$
$= - 2.303 \times 2 \times 298 lo g 1 0^{- 8}$
$= - 2.303 \times 2 \times 298 \times - 8 c a l$
$= 10980 c a l = 10.98 k c a l$

Q. The equilibrium constant Kp​ for a homogeneous gaseous reaction is 10−8. The standard Gibbs free energy change ΔG⊖ for the reaction (using R=2cal−1mol−1 ) is

10.98kcal

−1.8kcal

−4.1454kcal

+4.1454kcal