Consider the following reactions. In which case the formation of product is favoured by decrease in pressure? (1) CO2(g)+C(s)→2CO(g); ΔH=+172.5 kJ (2) N2(g)+3H2(g)→2NH3(g); ΔH=−91.8 kJ (3) N2(g)+O2(g)→2NO(g); ΔH=+181 kJ (4) 2H2O(g)→2H2(g)+O2(g);ΔH=484.6 kJ
2,3
3,4
2,4
1,4
A
1,4
B
2,4
C
3,4
D
2,3
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Solution
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If pressure is decreased, then equilibrium shift to more gas molecules side.
Here product is favoured if product gas mole are more than reactant gas mole.
(1) CO2(g)+C(s)⇌2CO
Here reactant gas mole= 1
Product gas moles= 2
If we reduce pressure, equilibrium shift to product side.
(4) 2H2O(g)⇌2H2(g)+O2(g)
Reactant gas moles= 2
Product gas moles= 3
If we reduce pressure, equilibrium shift to product side
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Q1
Consider the following reactions. In which case the formation of product is favoured by decrease in pressure? (1) CO2(g)+C(s)→2CO(g); ΔH=+172.5 kJ (2) N2(g)+3H2(g)→2NH3(g); ΔH=−91.8 kJ (3) N2(g)+O2(g)→2NO(g); ΔH=+181 kJ (4) 2H2O(g)→2H2(g)+O2(g);ΔH=484.6 kJ
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Q2
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