Two moles of an equimolar mixture of two alcohols R1-OH and R2-OH are esterified with 1 mole of acetic acid .If 80% of the acid is comsumed and the quantities of ester formed under eqilibrium are in the ratio of3:2,what is the value of the equlibrium constant for the esterification of R1-OH ?
R1-OH + R2-OH + 2CH3COOH ⇔CH3COOR1 + CH3COOR2 + 2H2O
2 moles 2 moles 1 mole 0 moles 0 moles
At equilibrium
0.8 moles of CH3COOH consumed
So it produced
0.8*3/5 = 0.48 moles of CH3COOR1
0.8*2/5 = 0.32 moles of CH3COOR2
Kc = [0.48] [0.32] [1.6] / [1.6] [1.6] [0.2] = 0.48