Q. If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, what will be the effect on the equilibrium position?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Increase the rate of reaction
Solution
According to Le Chatelier's Principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.
Q. What is the effect of decreasing the volume of the container on the equilibrium of the reaction 2N2O(g) ⇌ 2N2(g) + O2(g)?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Increase the rate of reaction
Solution
Decreasing the volume increases the pressure, shifting the equilibrium towards the side with fewer moles of gas. The left side has 2 moles (N2O) compared to 3 moles (N2 + O2), so it shifts to the left.
Q. What will happen to the equilibrium position of the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) when the pressure is increased?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on temperature
Solution
Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. Here, the right side has 2 moles (NH3) compared to 4 moles (N2 + 3H2), so the equilibrium shifts to the right.
