-Q- Calculate a - G- and b the equilibrium constant for the formation of NO 2 from NO and O 2 at 298 K NO g -1 - 2 O 2 g - NO 2 g where - f- NO 2-52-0 kJ - mol- f- NO -87-0 kJ - mol- f G- O 2-0 kJ - mol

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Characteristics of Equilibrium Constant

[[Q]] Calcula...

Question

[[Q]]

Calculate a) G°and b) the equilibrium constant for the formation of NO₂ from NO and O₂ at 298 K

where _fG° (NO₂) = 52.0 kJ/mol

_fG° (NO) = 87.0 kJ/mol

_fG° (O₂) = 0 kJ/mol

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Solution

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Similar questions

[[Q]]

Calculate a) G°and b) the equilibrium constant for the formation of NO₂ from NO and O₂ at 298 K

where _fG° (NO₂) = 52.0 kJ/mol

_fG° (NO) = 87.0 kJ/mol

_fG° (O₂) = 0 kJ/mol

Calculate a) ΔG°and b) the equilibrium constant for the formation of NO₂ from NO and O₂ at 298 K

where Δ_fG° (NO₂) = 52.0 kJ/mol

Δ_fG° (NO) = 87.0 kJ/mol

Δ_fG° (O₂) = 0 kJ/mol

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

Δ G^{0}

N O_{2}

O_{2}

N O + 1 / 2 O_{2} ⇌ N O_{2}

Δ_{f} G^{0} (N O_{2}) = 52.0 k J / m o l

Δ_{f} G^{0} (N O) = 87.0 k J / m o l

Δ_{f} G^{0} (O_{2}) = 0 k J / m o l

△ G^{\circ}

N O_{2}

N O

O_{2}

(1.365 \times 10^{6}) = 6.14

N O (g) + \frac{1}{2} O_{2} (g) ⇌ N O_{2} (g)

△ G^{\circ} (N O_{2}) = 52.0

△ G^{\circ} (N O) = 87.0

△ G^{\circ} (O_{2}) = 0

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