Question

Consider the equilibrium set up:
$2H_{2(g)}+C{O}_{(g)}\rightleftharpoons C{H}_{3}O{H}_{(g)}$
What will be the effect of the following on the equilibrium of the reaction?
(i) Addition of $H_2$
(ii) Addition of $C{H}_{3}OH$
(iii) Removal of $CO$
(iv) Removal of $C{H}_{3}OH$

	(i)	(ii)	(iii)	(iv)
(a)	Forward direction	Backward direction	Backward direction	Forward direction
(b)	Backward direction	Backward direction	Forward direction	Forward direction
(c)	Forward direction	Forward direction	Backward direction	Backward direction
(d)	Backward direction	Forward direction	Forward direction	Backward direction

• A. a
• B. b
• C. c
• D. d

Answer 1

Answer: (A)

(i) Increase in concentration of reactants favours forward reaction.
(ii) Increase in concentration of products favours backward reaction.
(iii) Removal of $CO$ will favour backward reaction (decrease in concentration of reactants).
(iv) Removal of $C{H}_{3}OH$ will favour forward reaction (increase in concentration of products).