KCET · Chemistry · Chemical Equilibrium
The yield of the products in the reaction, \(A_{2}(g)+2 B(g) \rightleftharpoons C(g)+Q\) kJ would be higher at
- A high temperature and high pressure
- B high temperature and low pressure
- C low temperature and high pressure
- D low temperature and low pressure
Answer & Solution
Correct Answer
(C) low temperature and high pressure
Step-by-step Solution
Detailed explanation
\(A_{2}(g)+2 B(g) \rightleftharpoons C(g)+Q k J\)
Obviously, the forward reaction is exothermic. Thus, according to Le-Chatelier's principle, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus, according to Le-Chatelier's principle an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other words high pressure will favour the formation of products.
Obviously, the forward reaction is exothermic. Thus, according to Le-Chatelier's principle, the lower is temperature, greater would be the yield of ammonia. Also, the forward reaction occurs with decrease in number of gaseous molecules. Thus, according to Le-Chatelier's principle an increase in pressure, will shift the equilibrium in a direction in which the number of gaseous molecules decreases. In other words high pressure will favour the formation of products.
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