When at equilibrium, which of the reactions below will shift to the right if the pressure is increased and the temperature is kept constant?
2SO3(g) ↔ 2SO2(g) + O2(g)
2CO2(g) ↔ 2CO(g) + O2(g)
2H2(g) + O2(g) ↔ 2H2O(g)
2NO(g) ↔ N2(g) + O2(g)
Explanation
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Discussions (14)
Increase in pressure of an equillibrum reaction favours the side with the lowest number of mole...so option C is correct
option C is correct... Note: when increasing pressure in a reaction it depends mostly on non gases. Hence, applying pressure in a reaction which will result in gases will therefore be lost to the surrounding.
C is correct
increase in volume= decrease in Pressure
decrease in Volume= increase in pressure
According to d gas laws.. Pressure is inversely proportional to volume. Therefore increase in pressure would bring about a decrease in d volume. Then d equation wit d forward reaction dat has d least mole is d answwer which is Option C.
