Question

2. What will happen to the number of moles of So, in equilibrium with SO2 and O, in the reaction in each of the following cases? 250,(8) 250.(8) + ($) a. Oxygen gas is added. b. In a rigid reaction container, the pressure is increased. e. The temperature is decreased the reaction is endothermic). d. Gaseous sulfur dioxide is removed. 3. An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction. At equilibrium, the concentrations are [H.] - 5.0 M. [Na] = 8.0 M, and (NH) - 4.0 M. What were the concentrations of en gas and hydrogen gas that were reacted initially?

Answer 1

Ans 2 :

According to Le Chatelier's principle , when a system at equilibrium is subjected to any change in reaction conditions , the reaction shifts in the direction where the equilibrium can be re-estabilished again.

So here :

a)

Oxygen is product here , so adding more oxygen to the system will shift the reaction to left increasing the number of moles of SO3.

b)

Increasing the pressure will cause the reaction to shift in the direction where pressure is less i.e. towards reactants. So the number of moles of SO3 will increase.

c)

Since the reaction is endothermic already , so decreasing the temperature will cause the reaction to move left , and hence the number of moles of SO3 will increase.

d)

SO2 is a product here , so removing SO2 will cause the reaction to move right and hence the number of moles of SO3 will decrease.