For N2g-O2g- 2NO2- - H - 66 kJ- the heat of formation in kJ of NO2 is -

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Heat of Formation

For N2g+O2g...

Question

For $N_{2} (g) + O_{2} (g) ⟶ 2 N O_{2}; Δ H = 66 k J$ , the heat of formation (in kJ) of $N O_{2}$ is ________.

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As per the reaction $N_{2} + 2 O_{2} \to 2 N O_{2} (g)$ , $Δ H = 66 K J$ the molar heat of formation of $N O_{2}$ is

C O_{2} (g) + C (s) \to 2 C O (g)

Δ H = + 172.5

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

Δ H = - 91.8

N_{2} (g) + O_{2} (g) \to 2 N O (g)

Δ H = + 181

2 H_{2} O (g) \to 2 H_{2} (g) + O_{2} (g); Δ H = 484.6

{N o}_{2}

[\frac{1}{2} N_{2 (g)} + O_{2 (g)} \to {N O}_{2 (g)}]

N_{2 (g)} + O_{2 (g)} \to 2 {N O}_{(g)}

y

2 {N O}_{(g)} + O_{2 (g)} \to 2 {N O}_{2 (g)}

z

C (s) + O_{2} (g) \to C O_{2} (g)

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

{N O}_{2}

[1 / 2 N_{2 (g)} + O_{2 (g)} \to {N O}_{2 (g)}]

N_{2 (g)} + O_{2 (g)} \to 2 {N O}_{(g)}

2 N O_{(g)} + O_{2 (g)} \to 2 {N O_{2}}_{(g)}

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