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Question

Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(i) COCl2(g)CO(g)+Cl2(g)
(ii) CH4(g)+2S2(g)CS2(g)+2H2S(g)
(iii) CO2(g)+C(s)2CO(g)
(iv) 2H2(g)+CO(g)CH3OH(g)
(v) CaCO3(s)CaO(s)+CO2(g)
(vi) 4NH3(g)+5O2(g)4NO(g)+6H2O(g)

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Solution

(i) The change in the number of moles of the gaseous species Δn=21=1.
When pressure is increased, the equilibrium reaction is affected. The direction of reaction will shift into backward direction.
(ii)The change in the number of moles of the gaseous species Δn=33=0.
When the pressure is increased, the equilibrium reaction is not affected.
(iii) The change in the number of moles of the gaseous species Δn=21=1.
When pressure is increased, the equilibrium reaction is affected. The direction of reaction will shift into backward direction.
(iv) The change in the number of moles of the gaseous species Δn=13=2.
When pressure is increased, the equilibrium reaction is affected. The direction of reaction will shift into forward direction.
(v) The change in the number of moles of the gaseous species Δn=10=1.
When pressure is increased, the equilibrium reaction is affected. The direction of reaction will shift into backward direction.
(vi) The change in the number of moles of the gaseous species Δn=109=1.
When pressure is increased, the equilibrium reaction is affected. The direction of reaction will shift into backward direction.

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