part A the answer is 6.5 but how do youCalculate the number of moles of all reac

Question

part A the answer is 6.5 but how do youCalculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 of acetic acid and 10.00 of ethanol.

The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25C: Part A How many moles of ethyl acetate are present in an equilibrium mixture that contains 3.6 mol of acetic acid, 6.4 mol of ethanol, and 12.0 moI of water at 25 C? part A the answer is 6.5 but how do youCalculate the number of moles of all reactants and products in an equilibrium mixture prepared by mixing 1.00 of acetic acid and 10.00 of ethanol.

Explanation / Answer

3.4 = x * 12 /(3.6*6.4) x = 6.52 3.4 = x^2/(1-x)/(10-x) solve for x

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