Based on le chatelier's principle, under what conditions would the yield of ch4(g) be maximized?

co2(g) + 4 h2(g) > ch4(g) + 2 h2o(g)

δhº = -165 kj/molrxn

high p and low t
low p and high t
high p and high t
low p and low t

High P and Low T

Where P is the Pressure and T is the Temperature.

Explanation:

1. High Pressure : The above chemical equation has the reactant and product sides.

The product side has total moles of 3 and reactant side has total moles of 4.

To obtain maximum yield in the production of CH4 , pressure must be high because it will favour the side the less number of moles(volume) which is the product side.

2.Low Temperature : The enthaply change indicated as negative shows it is an exothermic reaction. And for an exothermic reaction, the temperature must be lower so as to favor the forward reaction and to make up for the heat/energy loss.