Why does equilibrium reach faster when the pressure is increased?

I wonder why this view is wrong.
“a greater proportion of molecules in the mixture have energy greater than the activation energy”

I thought that as the pressure increases, the temperature increases and the kinetic energy of more molecules increases. Why is this view wrong?

(IMAT 2018 Q51)

Check this out: IMAT 2018 Q51 [Haber Process]

Since the question says that the temperature remains constant, this statement is untrue.

Increasing temperature and remaining other things constant can mean increase in KE of molecules and increase in pressure.

On the other hand, increasing pressure without any change in temperature does not always make KE to increase.

Oh my… I didn’t take into account the condition that the temperature is constant.
I guess I didn’t read the question properly
thank you so much :joy:

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