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Question

In the following reversible reaction 2SO2(g)+O2(g)2SO3(g), ΔH=+Q cal,
where Q is negative. Most suitable condition for a low production of SO3 is:

A
High temperature and high pressure
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B
High temperature and low pressure
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C
Low temperature and high pressure
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D
Low temperature and low pressure
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Solution

The correct option is B High temperature and low pressure
Given reversible reaction 2SO2(g)+O2(g)2SO3(g), ΔH=+Q cal

We need a low production of SO3 i.e. lower amount of product.
Since ΔH<0
The reaction is exothermic. For a high temperature, the reaction will proceed in backward direction, i.e. the reactant side. So, less SO3 will be formed.

Pressure:
Δng=23=1Δng<0
For a low pressure, the reaction will tend to go that side where number of gaseous moles increase. It increases in backward direction. So, for a low pressure more reactants are formed and less SO3 is formed.

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