At 573 K, the equilibrium constant for N2 (g) +3H2 (g) <--> 2NH3 (g) is 4.34 Ã10^-3. At 700 K, Kc=1.04Ã10^-4.

Is this an endothermic or exothermic reaction? Explain.
The formation of ammonia from nitrogen gas and hydrogen gas is an important industrial process. As you can see, the equilibrium constant for this reaction decreases as the temperature increases. Why then is the reaction performed at very high temperature? How do you think the yield of ammonia is maximized?

Question

At 573 K, the equilibrium constant for N2 (g) +3H2 (g) <--> 2NH3 (g) is 4.34 Ã10^-3. At 700 K, Kc=1.04Ã10^-4.

Is this an endothermic or exothermic reaction? Explain.
The formation of ammonia from nitrogen gas and hydrogen gas is an important industrial process. As you can see, the equilibrium constant for this reaction decreases as the temperature increases. Why then is the reaction performed at very high temperature? How do you think the yield of ammonia is maximized?

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