Question 7.30 At 473 K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. If decomposition is depicted as,
PCl5(g) <--->PCl3(g) + Cl2(g) ΔrH° = 124.0 kJmol–1
a) Write an expression for Kc for the reaction.
b) What is the value of Kc for the reverse reaction at the same temperature?
c) What would be the effect on Kc if (i) more PCl5 is added (ii) pressure is increased? (iii) The temperature is increased?
Class XI Equilibrium Page 227
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PCl5 <=> PCl3 + Cl2;Kc = 8.3 × 10^-3
(a) Kc = [PCl3][Cl2]/[PCl5]
(b) if reaction will be reverse then , equilibrium constant ( K'c) = 1/Kc = 1/{8.3 × 10^-3}
= 120.48
(c) equilibrium constant is constant at constant temperature hence, there is no effect on Kc when addition of PCl5.
(c) equilibrium constant is independent upon concentration of pressure. Hence, Kc doesn't change with pressure.
(d) this is an endothermic reaction hence, when increases in the temperature Kf increases . So, Kc = Kf/Kb increases.
(a) Kc = [PCl3][Cl2]/[PCl5]
(b) if reaction will be reverse then , equilibrium constant ( K'c) = 1/Kc = 1/{8.3 × 10^-3}
= 120.48
(c) equilibrium constant is constant at constant temperature hence, there is no effect on Kc when addition of PCl5.
(c) equilibrium constant is independent upon concentration of pressure. Hence, Kc doesn't change with pressure.
(d) this is an endothermic reaction hence, when increases in the temperature Kf increases . So, Kc = Kf/Kb increases.
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