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प्रश्न
Predict which of the following reaction will have the appreciable concentration of reactants and products:
- \[\ce{Cl2 (g) ⇌ 2Cl (g)}\] Kc = 5 ×10–39
- \[\ce{Cl2 (g) + 2NO (g) ⇌ 2NOCl (g)}\] Kc = 3.7 × 108
- \[\ce{Cl2 (g) + 2NO2 (g) ⇌ 2NO2Cl (g)}\] Kc = 1.8
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उत्तर
Following conclusions can be drawn from the values of Kc .
- Since the value of Kc is very small, this means that the molar concentration of the products is very small as compared to that of the reactants.
- Since the value of Kc is quite large, this means that the molar concentration of the products is very large as compared to that of the reactants
- Since the value of Kc is 1.8, this means that both the products and reactants have appreciable concentration.
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संबंधित प्रश्न
Write the expression for the equilibrium constant, Kc for each of the following reactions:
\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]
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\[\ce{Fe^{3+}(aq) + 3OH^-(aq) ⇌ Fe(OH)3(s)}\]
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\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]
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\[\ce{2NO(g) + Br2 (g) ⇌ 2NOBr (g)}\]
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\[\ce{NO(g) + 1/2 O_2 (g) <=> NO_2(g)}\]
where ΔfG⊝ (NO2) = 52.0 kJ/mol
ΔfG⊝ (NO) = 87.0 kJ/mol
ΔfG⊝ (O2) = 0 kJ/mol
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Some reactions are written below in Column I and their equilibrium constants in terms of Kc are written in Column II. Match the following reactions with the corresponding equilibrium constant
| Column I (Reaction) | Column II (Equilibrium constant) |
| (i) \[\ce{2N2 (g) + 6H2 (g) ⇌ 4NH3 (g)}\] | (a) `2K_c` |
| (ii) \[\ce{2NH3 (g) ⇌ N2 (g) + 3H2 (g)}\] | (b) `K_c^(1/2)` |
| (iii) \[\ce{1/2 N2 (g) + 3/2 H2 (g) ⇌ NH3 (g)}\] | (c) `1/K_c` |
| (d) `K_c^2` |
Match standard free energy of the reaction with the corresponding equilibrium constant.
| Column I | Column II |
| (i) ∆GΘ > 0 | (a) K > 1 |
| (ii) ∆GΘ > 0 | (b) K = 1 |
| (iii) ∆GΘ = 0 | (c) K = 0 |
| (d) K < 1 |
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\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]
the equilibrium constant is K1. The equilibrium constant is K2 for the reaction
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\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?
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\[\ce{NH3(g) <=> 1/2N2(g) + 3/2H2(g)}\]
In which one of the following equilibria, KP ≠ Kc?
