1. Tardigrade
  2. Question
  3. Chemistry
  4. Calculate Δ G for the given reaction at 298 K under given conditions: N 2 O 4(g)=2 NO 2(g) The reaction is carried out at 298 K and 20 bar. 5 moles each of N 2 O 4 and NO 2 are taken initially. (Δ GN2 O4°=100 kJ / mol , Δ GN2°=50 kJ / mol )

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Q. Calculate $\Delta G$ for the given reaction at $298\, K$ under given conditions :
$N _2 O _{4(g)}=2 NO _{2(g)}$
The reaction is carried out at $298\, K$ and $20$ bar. $5$ moles each of $N _2 O _4$ and $NO _2$ are taken initially.
$\left(\Delta G_{N_2 O_4}^{\circ}=100\, kJ / mol , \Delta G_{N_2}^{\circ}=50\, kJ / mol \right)$

Thermodynamics

Solution:

$\Delta G_{\text {Reaction }}=\Sigma \Delta G_{f(\text { Product })}^{\circ}-\Sigma \Delta G_{f(\text { Reactant })}^{\circ}$
$=2 \times 50-100=0$