Methanol, CH3OH, is produced on an industrial scale from carbon monoxide and hydrogen. At the temperatures used, gaseous methanol is formed according to the following thermochemical equation:
CO(g)+ 2H2(g) <---> CH3OH(g) �£H = -90Kj
1. State Le Chateliers principle and explain the following:
a)The effect that increasing the pressure will have on the equalibrium yield of menthanol
b) the effect of increasing the temperature will have on the equalibrium yield of menthanol
c) the effect of increasing the temperature will have on the rate of reaction
where appropriate, show clear understanding of how the Le Chatelier's principle applies
I will be happy to critique your thinking on this.
Le Chateliers principle states that If a system in a state of equilibrium is disturbed, it will undergo a change that shifts its equilibrium position in a direction that reduces the effect of the disturbance.
Therefore,
a)If you increase pressure on a gas you decrease the volume (boyles law), the reaction will shift in a direction to the side of the reaction with the fewer moles of gas in order to reduce pressure and bring the system back to equilibrium
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