JAMB - Chemistry (1999 - No. 22)
N\(_2\)O\(_4\)(g) ↔ 2NO\(_2\)(g). Increase in total pressure of the equilibrium reaction above will
produce more of NO2(g) in the mixture
convert all of N2O4(g) to NO2(g)
have no effect on the concentrations of NO2(g)and N2O4(g)
produce more of N2O4(g) in the mixture
Explanation
An increase in pressure on a system at equilibrium, according to Le Chatelier's principle, shifts the equilibrium towards the side with fewer moles of gas to relieve the stress of increased pressure.
In the above reaction, the side with the lesser number of moles of gaseous species is the reactant,N\(_2\)O\(_4\) with 1 mole as against the product side with 2 moles. Hence, an increase in total pressure will favour the side with the lesser number moles. This implies more N\(_2\)O\(_4\) will be produced.
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