goodbody02
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Carbon monoxide and hydrogen are used in the manufacture of methanol (CH^3OH). The reaction is reversible and can reach a position of dynamic equilibrium. CO(g) +2H^2(g) <=> CH^3OH(g) deltaH = -91KJ/mol
This reaction is carried out at a pressure of about 100 atmospheres and a temperature of 250'c

How would a decrease in temperature at constant pressure affect the amount of methanol in the equilibrium mixture? Explain your answer

How would an increase in pressure at constant temperature affect the amount of methanol in the equilibrium mixture? Explain your answer

Please someon answer this its the only question I cant do in my worksheet
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The Sikh Surgeon
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(Original post by goodbody02)
Carbon monoxide and hydrogen are used in the manufacture of methanol (CH^3OH). The reaction is reversible and can reach a position of dynamic equilibrium. CO(g) +2H^2(g) <=> CH^3OH(g) deltaH = -91KJ/mol
This reaction is carried out at a pressure of about 100 atmospheres and a temperature of 250'c

How would a decrease in temperature at constant pressure affect the amount of methanol in the equilibrium mixture? Explain your answer

How would an increase in pressure at constant temperature affect the amount of methanol in the equilibrium mixture? Explain your answer

Please someon answer this its the only question I cant do in my worksheet
Decrease temp = Shift equilibrium right as forward reaction is exothermic. This increases temp and opposes the decrease in temp
increase amount of methanol

Increase pressure = shift equilibrium right as this is the side with fewer moles of gas (left has 2 moles and right has 1 mole) this will decrease pressure opposing the increase in pressure
increase amount of methanol
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