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Calorimetry

In which of t...

Question

In which of the following reactions the formation of product is favoured by decreasing the temperature or volume?

2 {S O}_{3 (g)} ⇌ 2 S_{(g)} + 3 O_{2 (g)}, - q

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N_{2 (g)} + O_{2 (g)} ⇌ 2 {N O}_{(g)}, - q

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4 {N H}_{3 (g)} + 5 O_{2 (g)} ⇌ 4 {N O}_{(g)} + 6 {H_{2} O}_{(g)}, Δ H

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2 {N O}_{(g)} + O_{2 (g)} ⇌ 2 {N O}_{2 (g)}, Δ H

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Solution

The correct option is B $2 {N O}_{(g)} + O_{2 (g)} ⇌ 2 {N O}_{2 (g)}, Δ H$ is $-$ ve
When the volume of the system is changed, the partial pressures of the gases change. Decrease in pressure by increasing volume, the equilibrium of the reaction would shift to the direction where the greater number of moles than the other side. $2 {N O}_{(g)} + O_{2 (g)} ⇌ 2 {N O}_{2 (g)} Δ H$ -ve is a exothermic reaction would be favoured by decrease in temperature. Product side has less number of moles thus decrease in volume or pressure will favour the reaction.

Suggest Corrections

Similar questions

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

Δ H = 181

2 C O_{2} (g) \to 2 C O (g) + O_{2} (g); Δ H = 566

H_{2} (g) + I_{2} (g) \to 2 H I (g); Δ H = - 94

H_{2} (g) + F_{2} (g) \to 2 H F (g); Δ H = - 541

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

\begin{matrix} List - I & List - II (I) Dissociation of N_{2} O_{4} (g) : & (P) Increases with N_{2} O_{4} (g) ⇌ 2 N O_{2} (g); & temperature Δ H = + 57.0 k J (II) Oxidation of N H_{3} (g) : & (Q) Decreases with 4 N H_{3} (g) + 5 O_{2} ⇌ 4 N O (g) + 6 H_{2} O (g); & pressure Δ H = - 900.0 k J (III) Oxidation of nitrogen: & (R) Increases with N_{2} (g) + O_{2} (g) ⇌ 2 N O (g); & addition of inert Δ H = + 180.0 k J & gas at constant pressure (IV) Formation of N O_{2} (g) : & (S) Decreases with N O (g) + O_{3} (g) ⇌ N O_{2} (g) + O_{2} (g); & temperature Δ H = - 200.0 k J (T) K_{p} = K_{c} (U) K_{p} = K_{c} (R T)^{1} \end{matrix}

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g) Δ H = Q c a l s

N O

4 N H_{3} (g) + 5 O_{2} (g) \to 4 N O (g) + 6 H_{2} O (l) Δ H = - 904 k J . . . (1)

2 N O (g) + O_{2} (g) \to 2 N O_{2} (g) Δ H = - 112 k J . . . (2)

3 N O_{2} (g) + H_{2} O (l) \to 2 H N O_{3} (a q) + N O (g) Δ H = - 140 k J . . . (3)

(i n kJ/mole)

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