Chapter 15, Problem 15.96SP

Interpretation Introduction

(a)

Interpretation:

The number of moles of Ethyl acetate in an equilibrium mixture needs to be determined.

Concept introduction:

A chemical reaction is said to be in equilibrium if there is no further change in its concentration takes place with time. The equilibrium constant is defined as ratio of equilibrium concentration/molarity of product to reactant reaction raised to the power of the respective stochiometric coefficient in the equilibrium reaction.

For a general equilibrium reaction as follows:

$aA+bB\rightleftharpoons cC+dD$

The expression for equilibrium constant can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

Here, A, B, C, D is concentrations of reactants and products and a, b, c, d is the respective stoichiometric coefficient.

For 1 L of volume, Kc can also be written on the basis of number of moles.

Number of moles can be calculated from molarity of solution as follows:

$n=M\times V\left(L\right)$

Here, M is molarity and V is volume of solution in L.

Interpretation Introduction

(b)

Interpretation:

The number of moles of all product and reactants as acetic acid, ethanol, ethyl acetate and water at equilibrium needs to be determined.

Concept introduction:

A chemical reaction is said to be in equilibrium if there is no further change in its concentration takes place with time. The equilibrium constant is defined as ratio of equilibrium concentration/molarity of product to reactant reaction raised to the power of the respective stochiometric coefficient in the equilibrium reaction.

For a general equilibrium reaction as follows:

$aA+bB\rightleftharpoons cC+dD$

The expression for equilibrium constant can be represented as follows:

$K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

Here, A, B, C, D is concentrations of reactants and products and a, b, c, d is the respective stoichiometric coefficient.

For 1 L of volume, Kc can also be written on the basis of number of moles.

Number of moles can be calculated from molarity of solution as follows:

$n=M\times V\left(L\right)$

Here, M is molarity and V is volume of solution in L.