Problem: Consider the following reaction at equilibrium in a closed container.4 NH3 (g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) ΔH = +64.5 kJ/molIncreasing the temperature of the reaction vessel will __________ the NH3 partial pressure.  A) increaseB) decrease C) not change

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We’re being asked to determine what will happen to the NH3 partial pressure when the temperature is increased. 


4 NH3 (g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g)   ΔH = +64.5 kJ/mol


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.


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Problem Details

Consider the following reaction at equilibrium in a closed container.

4 NH3 (g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) ΔH = +64.5 kJ/mol

Increasing the temperature of the reaction vessel will __________ the NH3 partial pressure.  

A) increase

B) decrease 

C) not change



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What scientific concept do you need to know in order to solve this problem?

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.