Given the following reactionsI - N2g - 2O2g - 2NO4g- - HI - 16-18 kcalII - N2g - 2O2g - N2O4g- - HII - 2-31 kcalWhich amongs NO2 gand N2O4g is more stable-

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Heat of Formation

Given the fol...

Question

Given the following reactions
I : $N_{2} (g) + 2 O_{2} (g) \to 2 N O_{4} (g), Δ H_{I} = 16.18 k c a l$
II : $N_{2} (g) + 2 O_{2} (g) \to N_{2} O_{4} (g), Δ H_{I I} = 2.31 k c a l$
Which amongs $N O_{2} (g)$ and $N_{2} O_{4} (g)$ is more stable?

N_{2} O_{4} (g)

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N O_{2} (g)

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both of them are equally stable

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none of them are stable

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Solution

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I . N_{2} (g) + 2 O_{2} (g) ⟶ 2 N O_{2} (g); Δ H_{I} = 16.18 kcal

I I . N_{2} (g) + 2 O_{2} (g) ⟶ N_{2} O_{4} (g); Δ H_{I I} = 2.31 kcal

25^{\circ} C

N_{2} (g) + 2 O_{2} (g) \to 2 N O_{2} (g); △ H = 16.18 k c a l

N_{2} (g) + 2 O_{2} (g) \to N_{2} O_{4} (g); △ H = 2.31 k c a l

N O_{2}

N_{2} O_{4}

N O_{2}

25^{\circ} C

(13.87 k c a l, N_{2} O_{4}

(I) N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N_{2} O (g); K_{C} = 2.7 \times 10^{- 18}

(I I) N_{2} O_{4} (g) ⇌ 2 N O (g); K_{C} = 4.6 \times 10^{- 3}

(I I I) \frac{1}{2} N_{2} (g) + O_{2} (g) ⇌ N O_{2} (g) K_{C} 4.1 \times 10^{- 9}

2 N_{2} O (g) + 3 O_{2} (g) ⇌ 2 N_{2} O_{4} (g), K_{C}

m o l^{- 1}

N O_{2} (g)

N_{2} O_{4} (g)

N O_{2}

2 N O_{2} (g) = N_{2} O_{4} (g)

\frac{K_{p}}{K_{c}}

300 K

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

[A t 300 K, R T = 24.62 d m^{3} a t m m o l^{- 1}]

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