Consider the following equation : \(2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g}), \Delta \mathrm{H}=-190 \mathrm{~kJ}\) The number of factors which will increase the yield of \(\mathrm{SO}_{3}\) at equilibrium from the following is A. Increasing temperature B. Increasing pressure C. Adding more \(\mathrm{SO}_{2}\) D. Adding more \(\mathrm{O}_{2}\) E. Addition of catalyst

JEE Main · 2023 · 30 Jan 2023 · Shift 2 · Equilibrium

Consider the following equation :

2 SO_{2} (g) + O_{2} (g) ⇌ 2 SO_{3} (g), Δ H = - 190 kJ

The number of factors which will increase the yield of

SO_{3}

at equilibrium from the following is
A. Increasing temperature
B. Increasing pressure
C. Adding more

SO_{2}

D. Adding more

O_{2}

E. Addition of catalyst

Answer: 3

Solution

Each change is weighed against this exothermic, mole-reducing equilibrium. Raising the temperature favours the reverse, heat-absorbing direction and lowers the yield, so it does not help. Adding a catalyst hastens both directions equally and leaves the position of equilibrium, and the yield, unchanged. Raising the pressure drives the system towards the side of fewer gas molecules, which is the product side, and raises the yield; supplying more sulphur dioxide and supplying more oxygen each add a reactant and likewise push the reaction forward. Three of the listed changes raise the yield of sulphur trioxide.

JEE Main · 2023 · 30 Jan 2023 · Shift 2 · Integer answer

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JEE Main · 2023 · 30 Jan 2023 · Shift 2 · Equilibrium

Solution

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