For which of the following reaction mixtures at equilibrium would reducing the v

Question

For which of the following reaction mixtures at equilibrium would reducing the volume of the container at constant temperature cause the equilibrium to shift toward the products? a. SrCO_3 (s) doubleheadarrow SrO (s) + CO_2 (g) b. C (s) + CO_2 (g) doubleheadarrow 2CO (g) c. CO(g) + H_2O (g) doubleheadarrow CO_2 (g) + H_2 (g) d. PCl_5 (g) doubleheadarrow PCl_3 (g) + Cl_2 (g) e. 2NO_2 (g) doubleheadarrow N_2O_4 (g) H_2 (g) + I_2 (g) doubleheadarrow 2HI (g) Delta H 0 > 0. Which of the following changes to the equilibrium system represented above will increase the quantity of HI (g) in the equilibrium mixture? I. Adding H_2 (g) II: Increasing the temperature III: Decreasing the pressure a. I only b. III only c. I & II only d. II & III only e. I, II & III

Explanation / Answer

9. e

Explanaton: On reducig the volume of the container the pressure of the container increases, so if delta ng = +ve the yield of the product decreases whereas if ng = -ve the yield of the product increases. delta ng = no of moles of gaseous products - no of moles of gaseous reactants.

a) the equilibrium will shift towards reactants. Because delta ng = 1 [CO2(g) is the only gaseous product and

no gaseous reactants.]

b) the equilibrium will shift towards reactants. Because delta ng = 2 -1 =1

c) It will not show any effect on the equilbrium because delta ng = (1+1) - (1+1) =0

d)   the equilibrium will shift towards reactants. Because delta ng = (1 + 1) - 1 = 1

e)  the equilibrium will shift towards products. Because delta ng = 1 - 2 = -1

10. c

Explanation: delta ng = 0 so no effect of pressure on equilibrium

delta H >0 the reaction is endothermic so on increasing the temperature the equilibrium will shift towards products.

On adding reactant the equilibrium will shift towards products. So the option is I and II.

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