Calculate Δ G0 the equilibrium constant for the formation of NO2 fr

1.	Calculate Δ G0 the equilibrium constant for the formation of NO2 from NO and O2 at 298 K NO(g)+12O2(g)↔NO2(g) Where: ΔfG∘ (NO2)=52.0kJ/molΔfG∘ (NO)=87.0kJ/molΔfG∘ (O2)=0kJ/mol
Answer» Calculate $Δ G^{0}$ the equilibrium constant for the formation of $N O_{2}$ from NO and $O_{2}$ at 298 K $N O (g) + \frac{1}{2} O_{2} (g) \leftrightarrow N O_{2} (g)$ Where: $Δ_{f} G^{\circ} (N O_{2}) = 52.0 k J / m o l Δ_{f} G^{\circ} (N O) = 87.0 k J / m o l Δ_{f} G^{\circ} (O_{2}) = 0 k J / m o l$

Calculate Δ G0 the equilibrium constant for the formation of NO2 from NO and O2 at 298 K NO(g)+12O2(g)↔NO2(g) Where: ΔfG∘ (NO2)=52.0kJ/molΔfG∘ (NO)=87.0kJ/molΔfG∘ (O2)=0kJ/mol

Answer»

Calculate

$Δ G^{0}$

the equilibrium constant for the formation of $N O_{2}$ from NO and $O_{2}$ at 298 K
$N O (g) + \frac{1}{2} O_{2} (g) \leftrightarrow N O_{2} (g)$

Where:
$Δ_{f} G^{\circ} (N O_{2}) = 52.0 k J / m o l Δ_{f} G^{\circ} (N O) = 87.0 k J / m o l Δ_{f} G^{\circ} (O_{2}) = 0 k J / m o l$