Answer
a) No effect
b) Shift towards right i.e. in the forward direction '
c) Shift towards right i.e. in the forward direction
d) Shift towards right i.e. in the forward direction
e) No effect
Work Step by Step
Write the equilibrium expression of the reaction
$C(s) + H_{2}O(g) \leftrightharpoons CO(g) +H_{2}(g)$
Equilibrium constant$ k_{eq} = \frac{[CO][H_{2}]}{[H_{2}O]}$
Now, if a chemical system is disturbed at equilibrium, the system minimizes the disturbance by shifting right or left direction (Le Chatelier's principle).
a) Adding more C to the reaction mixture will have no effect on the system. This is because: here the state of C is Solid. So, increasing or decreasing the concentration of C in the system will have no effect in the equilibrium system.
b) If we add more $H_{2}O$ to the reaction mixture the concentration of $H_{2}O$ increases. So, to minimize the disturbance of the system at equilibrium, the concentration of products should also be increased. This can happen if the forward reaction rate favored i.e. the reaction shifts towards right.
c) If we raised the temp. of the reaction mixture, the reaction will shift towards right. This is because: this is an endothermic reaction. That means heat is absorbed in forward reaction. So, if we increase temp. of the reaction, the extra heat must be absorbed by the system to minimize the disturbance. So, the extra heat will be absorbed if the reaction shifts toward right i.e. in the forward direction.
d) If we increase the volume of the reaction mixture, the pressure of the system is decreased. To minimize this disturbance, the reaction shifts toward the direction where there are more moles of gas particles. Now, no. of moles of gas particles at left is equal to 1 and at right is equal to 2. So, the reaction will shift towards right to minimize the disturbance.
e) Adding a catalyst to the reaction mixture will have no effect on the equilibrium system. Catalysts do not disturb the equilibrium of the system.
