Question

In the esterification $C_2{H}_{5}OH\left(l\right)+{CH}_{3ke}COOH\left(l\right)\rightleftharpoons {CH}_{3}COO{C}_2{H}_{ta5}\left(l\right)+H_{2}O\left(l\right)$ an equimolar mixture of alcohol and acid taken initially yields under equilibrium,the water with mole fraction=0.333.calculate the equilibrium constant.

Answer 1

$C_2{H}_{5}OH+{CH}_{3}COOH\rightleftharpoons {CH}_{3}COO{C}_2{H}_5+H_{2}O$

$1$ $1$ $-$ $-$

$1-x$ $1-x$ $x$ $x$

$x=0.333$

$K_C=\frac{\left[{CH}_{3}COO{C}_2{H}_5\right]\left[H_{2}O\right]}{\left[C_2{H}_{5}OH\right]\left[{CH}_{3}COOH\right]}$

$=\frac{{\left(0.333\right)}^2}{{\left(0.667\right)}^2}=0.25$