Problem: For the gas phase reaction N2 + 3 H2 ⇌ 2 NH3 ΔH° = -92 kJ for the forward reaction. In order to decrease the yield of NH3, the reaction should be runa. at high P, low T.b. at low P, high T.c. at high P, high T.d. at low P, low T.

FREE Expert Solution

We’re being asked to identify the condition in order to decrease the yield of NH3 for the gas-phase reaction:

N2 + 3 H2 ⇌ 2 NH3          ΔH° = -92 kJ



According to Le Chatelier’s Principle, if a system (chemical reaction) is at equilibrium and we disturb it, then the system will readjust to maintain its equilibrium state.



Since the reaction is exothermic, ΔH = (–), heat is given off as a product:

N2(g) + 3 H2(g) ⇌ 2 NH3(g) + heat


Now, let’s look at the effect of changing pressure and temperature on the reaction.


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Problem Details

For the gas phase reaction N2 + 3 H2 ⇌ 2 NH3 ΔH° = -92 kJ for the forward reaction. In order to decrease the yield of NH3, the reaction should be run

a. at high P, low T.
b. at low P, high T.
c. at high P, high T.
d. at low P, low T.

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Our tutors have indicated that to solve this problem you will need to apply the Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.