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5J13 7th Ed

Posted: Mon Jan 21, 2019 4:06 pm
by Summer de Vera 2C
Why is it that less ammonia will be formed? Isn't the reaction endothermic, meaning that the products (ammonia) will be favored?

Re: 5J13 7th Ed

Posted: Mon Jan 21, 2019 4:32 pm
by Gillian Ward 1F
Looking at the equilibrium constants of each of the reactions at their respective temperatures, the equilibrium constant for the reaction at 700. K is smaller than the constant at 600. K. This tells us that the reactants are favored more in the higher temperature.

Re: 5J13 7th Ed

Posted: Mon Jan 21, 2019 8:09 pm
by Matthew Choi 2H
You're confusing exothermic/endothermic with a mere change in temperature. Just because they heat the mixture from 600 to 700 doesn't tell you anything about the reaction being exothermic/endothermic. Therefore, you can answer the question by looking at the k values that give you for each temperature. Since the k value at 700 K is smaller than the k value at 600 K, you deduct that there will be less products (NH3) formed when you increase the temperature.