Question

.   Consider the following equilibrium: 2 NO2 (g) + O2 (g) ⇌ 2 NO3 (g) +...

.   Consider the following equilibrium:

2 NO2 (g) + O2 (g) ⇌ 2 NO3 (g) + heat.

(A)   How would the equilibrium shift if extra NO2 were added?

(B) How would the equilibrium shift if O2 were removed?

(C) How would you change the temperature to cause a shift to the products?

(D) How would you change the pressure/volume to cause a shift to the reactants?

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Homework Answers

Answer #1

2 NO2 (g) + O2 2 NO3 (g) + heat

a) If extra NO2 is added, then equilibrium will shift in forward direction to counteract the change ( i.e to decrease concentration of NO2) and to re-establish equilibrium ( according to Le Chatelier Principle).

b) If O2 is removed then equilibrium will shift in reverse direction in order to increase O2.

c) As, heat is product so the given reaction is exothermic. Exothermic reaction are favoured at low temperature. So, when temperature is decreased , equilibrium will shift in forward direction.

d) When volume is increased and pressure is decreased, equilibrium shift from less number of moles to more number of moles (as it can now have more moles because of increased volume).

In the given reaction, moles of reactant is 3 and moles of product is 2. Therefore, on increasing volume, equilibrium will shift to reverse direction i.e shift to reactant.

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