Acetic acid can be manufactured by combining methanolwith carbon monoxide, an example of a carbonylationreaction: CH3OH(l) + CO(g)----->CH3COOH(l) (a) Calculate the equilibrium constant for the reaction at25 °C. (b) Industrially, this reaction is run at temperaturesabove 25 °C. Will an increase in temperature produce anincrease or decrease in the mole fraction of acetic acid atequilibrium? Why are elevated temperatures used? (c) Atwhat temperature will this reaction have an equilibriumconstant equal to 1? (You may assume that ΔH° and ΔS ° aretemperature independent, and you may ignore any phasechanges that might occur.)

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