5J13 7th Ed

Moderators: Chem_Mod, Chem_Admin

Summer de Vera 2C
Posts: 65
Joined: Fri Sep 28, 2018 12:16 am

5J13 7th Ed

Postby Summer de Vera 2C » Mon Jan 21, 2019 4:06 pm

Why is it that less ammonia will be formed? Isn't the reaction endothermic, meaning that the products (ammonia) will be favored?

Gillian Ward 1F
Posts: 61
Joined: Fri Sep 28, 2018 12:27 am

Re: 5J13 7th Ed

Postby Gillian Ward 1F » Mon Jan 21, 2019 4:32 pm

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.

Matthew Choi 2H
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: 5J13 7th Ed

Postby Matthew Choi 2H » Mon Jan 21, 2019 8:09 pm

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.

Return to “Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions”

Who is online

Users browsing this forum: No registered users and 1 guest