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Question
At 473 K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. If decomposition is depicted as,
\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\] ΔrH° = 124.0 kJmol–1
What would be the effect on Kc if
- more PCl5 is added
- pressure is increased?
- The temperature is increased?
Solution
- Kc would remain the same because in this case, the temperature remains the same.
- Kc is constant at constant temperature. Thus, in this case, Kc would not change.
- In an endothermic reaction, the value of Kc increases with an increase in temperature. Since the given reaction in an endothermic reaction, the value of Kc will increase if the temperature is increased.
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At 473 K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5is 8.3 ×10-3. If decomposition is depicted as,
\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\] ΔrH° = 124.0 kJmol–1
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At 473 K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5is 8.3 ×10-3. If decomposition is depicted as,
\[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\] ΔrH° = 124.0 kJmol–1
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