N2O4(g) ↔ 2NO2(g) ΔH = +ve
In the reaction above, an increase in temperature will
increase the value of the equilibrium constant
decreases the value of the equilibrium constant
increase in the reactant production
shift the equilibrium to the left
Explanation
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According to le chatelier's principle,in an endothermic rxn increase in temp favours forward rxn,thus equilibruim constant increases.A is the correct option.
For the given exothermic reaction N2O4 2NO2, the equilibrium will tend to shift towards the direction of the reaction that absorbs heat if the temperature is increased, and towards the direction of the reaction that releases heat if the temperature is decreased. The direction of the equilibrium will also tend to shift towards the side with fewer gas molecules if the pressure is increased, and towards the side with more gas molecules if the pressure is decreased.
Therefore, to determine the conditions that would produce the highest equilibrium yield of N2O4, we need to consider the effect of temperature and pressure on the equilibrium.
We know that the forward reaction is exothermic, which means it releases heat. Therefore, according to Le Chatelier's Principle, a low temperature would favor the forward reaction while a high temperature would favor the backward reaction.
On the other hand, the equilibrium shifts towards the side with fewer gas molecules when the pressure is increased, and towards the side with more gas molecules when the pressure is decreased. For this reaction, the forward reaction produces two moles of NO2 and the reverse reaction produces one mole of N2O4, which means that the forward reaction leads to an increase in the number of gas molecules. Therefore, decreasing the pressure would favor the forward reaction.
Now let's consider each option:
A) Low temperature and high pressure - This condition would favor the backward reaction according to both the temperature and pressure effects. Since both effects work against the forward reaction, this condition will produce a low equilibrium yield of N2O4.
B) Low temperature and low pressure - The low temperature would favor the forward reaction, but the low pressure would work against it. The net effect would depend on which effect is stronger, but overall it is likely that the yield of N2O4 would be lower than in the options with higher temperature and lower pressure.
C) High temperature and low pressure - The high temperature would favor the backward reaction, but the low pressure would favor the forward reaction. Since the forward reaction produces more gas molecules, it is likely that this condition would result in a higher equilibrium yield of N2O4 compared to options A and B.
D) High temperature and high pressure - The high temperature would favor the backward reaction, while the high pressure would work against it. This condition would produce a lower yield of N2O4 compared to option C.
Therefore, option C, high temperature and low pressure, will likely produce the highest equilibrium yield of N2O4. 
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