Esterification reaction given as ${\mathrm{RCOOH}}_{\left(aq\right)}+R^1{\mathrm{OH}}_{\left(aq\right)}\rightleftharpoons RCOO{R}_{\left(aq\right)}^1+H_2{O}_{\left(l\right)}$ .At same temperature diluting the equilibrium reaction with more water, then what change will be observed compared with equilibrium values?

$\text{ Reaction quotient }=\frac{\left[RCOO{R}^1\right]\left[H_{2}O\right]}{\left[RCOOH\right]\left[R^{1}OH\right]}$i

With dilution (by adding water), product side concentration increases and r_b dominating than r_{f ,  (temporarily) .} So equilibrium position will shifts from right to left. therefore no of moles of   RCOOH increases.