Ammonia is produced by the Haber process according to the following reaction. N2(g) + 3H2(g) 2NH3(g) DH is negative
(a) State the equilibrium constant expression for the above reaction.
(b) State and explain the effect on the value of Kc when the temperature is increased
(C) Explain why a catalyst has no effect on the position of equilibrium.
Answers
Answer:
A
Explanation:
because Nitrogen increased the temperature
Answer:
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Question
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In the manufacture of ammonia by Haber's process, N
2
(g)+3H
2
(g)⇋2NH
3
(g)+92.3kJ. Which of the following conditions is unfavourable?
Hard
Solution
verified
Increasing the temperature
The process of manufacturing of ammonia is an exothermic process,
On increasing temperature, the reaction will try to move in backward direction to neutralize its effect given by Le chatelier principle.
Hence, increasing the temperature becomes unfavourable condition for manufacturing ammonia.
Explanation:
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