Answer to Question #125901 in Inorganic Chemistry for Anelisa

Question #125901
For the reaction 4NH3(g) + 3O2(g)= 2N2(g)+ 6H2O(l), ∆H<0. How will the amount of ammonia at equilibrium be affected by
1 Removing O2
2 Adding N2
3 Adding H2O
4 Decreasing the pressure
5 increasing the temperature
Expert's answer

1 Removing O2

Increased! If oxygen is removed, the equilibrium shifts toward the reactants, producing more ammonia.

2 Adding N2

Increased! If more nitrogen gas is added it shifts the equilibrium towards the reactants again, causing more ammonia to build up.

3 Adding H2O

Increased! Same effect as for adding N2, addition of more products causes the shift towards the reactants.

4 Decreasing the pressure

Decreased! We have 7 mol of reactants vs 8 mol of products, so the products cause higher pressure in the system. If we decrease the pressure, system counteracts to the change producing more products, and reducing amount of ammonia.

5 Increasing the temperature

Increased! Heat is produced in this reaction (exothermic reaction). So additional temperature rise shifts the equilibrium towards the reactants, thus more ammonia is produced.

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