Question #d34eb

1 Answer
Jun 3, 2017

Adding heat and removing H2


The reaction producing CH3OH(g) is exothermic (it releases heat), so according to Le Chatelier's principle, if you increase the heat of the system, the system will act to oppose this increase in temperature and favour the endothermic (reverse) reaction.

If H2(g) is removed from the system, it will act to oppose the decrease in the concentration of H2(g), by favouring the reverse reaction which produces H2(g), and the concentration of CH3OH(g) will decrease.

Removing H2(g) would temporarily increase the value of Kp, decreasing the value of the denominator in the equation, and so when the concentration of H2(g) is increased again, the correct value of Kp will be restored.