Given that the following reaction is exothermic, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of N2O4(g) molecules? 2NO2(g) ⇌ N2O4(g) What observation would indicate that the reaction is at equilibrium in a closed container?
a. Increasing container volume and increasing temperature
b. Increasing container volume and decreasing temperature
c. Decreasing container volume and increasing temperature
d. Decreasing container volume and decreasing temperature
e. Changing volume or temperature will not affect the number of gas molecules present at equilibrium
Ans : d) decreasing container volume and decreasing temperature
Decreasing the volume of container increases the pressure in reaction mixture. So the reaction moves in a direction where the equillibrium can be re-estabilished. The pressure is less in the products side , so the decreasing volume will shift the equillibrium in right forming more N2O4.
After the reaction has reached its equillibrium state , there is no visible change in the concentration of any reactant or products , this indicates that the reaction is at equillibrium in a closed container.
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