Consider the equilibrium reaction represented by the equation: 2SO2(g) + O2(g) ⇌ 2SO3(g) ∆H = - 197 kJmol-1. At equilibrium, increase in the total pressure of the system brings about
decrease in rate of the reaction of the system
decrease in temperature of the system
increase in temperature of SO3
increase in concentration of SO2
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firstly, pressure aFFECTS gases only based on their number of moles. ( if number of mole of reactant is equal to number of mole of product, pressure has no effect egardless ) In this case the number of mole of reactant is greater than that of product so increase in pressure favours forward NOW, to temperature , it only has effect on endothermic and exothermic reactions . in endo, increase in temperature favours forward and vice versa BUT in exo, increase in temperature favours backward . LET'S reason ..... increase in pressure favours forward what form of temperature in exo will favour forward ( YES decrese in temperature, ) what of increase in temperature of reactant , it favours itself so only an increase in SO3 among the option favours itself
The selected answer is wrong:
According to le chateliers principle increase in pressure makes the equilibrium to shift to the right, from the equation below increase in pressure will increase the volume of so3 since there is reduction in volume from left to right which favours the product side. Thank you
REF: Check: comprehensive chemistry page 151 or lam
lard chemistry
Myschool is correct! Increase in total pressure will favour forward reaction! Which leads to more gas molecules being pushed to the right! Increase in pressure, as a result of the new gas molecules will bring about a rise in temperature of the reactants.
