1. Tardigrade
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  3. Chemistry
  4. The standard Gibbs free energy change (Δ G°) at 25°C for the dissociation of N2O4(g) to NO2(g) is (given, equilibrium constant = 0.15, R = 8.314 J/K/mol)

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Q. The standard Gibbs free energy change $(\Delta G^\circ)$ at 25$^{\circ}$C for the dissociation of $N_2O_4(g)$ to $NO_2(g)$ is (given, equilibrium constant = $0.15, R = 8.314 \, J/K/mol)$

WBJEEWBJEE 2013Thermodynamics

Solution:

$\Delta G^{\circ}=-2.303 \,R T \log K$
$=-2.303 \times 8.314 \times 298 \times \log 0.15 $
$=-2.303 \times 8.314 \times 298 \times(-0.82) $
$=4678.7 \,J =4.67\, kJ $