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Acetic acid can be manufactured by combining methanol with carbon monoxide, an example of a carbonylation reaction: CH3 OH(l) CO(g) ⟶CH3 COOH(l) (a) Calculate the equilibrium constant for the reaction at 25^∘ C .(𝐛) Industrially, this reaction is run at temperatures above 25^∘ C . Will an increase in temperature produce an increase or decrease in the mole fraction of acetic acid at equilibrium? Why are elevated temperatures used? (c) At what temperature will this reaction have an equilibrium co

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The equation for this reaction is: CH3OH(g) CO(g) -> CH3COOH(g). If ethanol is present in excess, how many moles of CO(g) are required to produce 16.6 moles of acetic acid?

State the Function of Cone, Sulphuric Acid in the Laboratory Preparation of Carbon Monoxide from Oxalic Acid. - Chemistry | Shaalaa.com

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