Chapter 17, Problem 17.82P

(a)

Interpretation Introduction

Interpretation:

The given equilibrium system is,

  ${\text{CO}}_{\text{2}}{}_{\text{(g)}}{\text{ + Ca(OH)}}_{\text{2(s)}}\rightleftharpoons {\text{CaCO}}_{\text{3(s)}}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ΔH}}^{\text{°}}\text{= -113 kJ}$

On decrease in temperature at constant pressure, ${\text{CaCO}}_{\text{3}}$ forms more or not has to be given.

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

The reactions of heat are of two types:

1. 1. Exothermic reaction – releases heat
2. 2. Endothermic reaction – absorbs heat

Change in equilibrium due to temperature changes:

If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.

If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.

(b)

Interpretation Introduction

Interpretation:

The given equilibrium system is

  ${\text{CO}}_{\text{2}}{}_{\text{(g)}}{\text{ + Ca(OH)}}_{\text{2(s)}}\rightleftharpoons {\text{CaCO}}_{\text{3(s)}}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ΔH}}^{\text{°}}\text{= -113 kJ}$

On increase in volume at constant temperature, ${\text{CaCO}}_{\text{3}}$ forms more or not has to be given.

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

Change in equilibrium due to pressure changes:

On decrease in the system volume, the equilibrium shifts towards fewer moles of gas, because, for gases,

  $\text{decrease in volume = increase in pressure}\text{.}$

On increase in the system volume, the equilibrium shifts towards more moles of gas, because, for gases,

  $\text{increase in volume = decrease in pressure}\text{.}$

(c)

Interpretation Introduction

Interpretation:

The given equilibrium system is

  ${\text{CO}}_{\text{2}}{}_{\text{(g)}}{\text{ + Ca(OH)}}_{\text{2(s)}}\rightleftharpoons {\text{CaCO}}_{\text{3(s)}}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ΔH}}^{\text{°}}\text{= -113 kJ}$

On increase in partial pressure of ${\text{CO}}_{\text{2}}$, ${\text{CaCO}}_{\text{3}}$ forms more or not has to be given.

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

Change in equilibrium due to pressure changes:

On increase in the system pressure, the equilibrium shifts towards fewer moles of gas, because, for gases,

  $\text{increase in pressure = decrease in volume}\text{.}$

On decrease in the system pressure, the equilibrium shifts towards more moles of gas, because, for gases,

$\text{decrease in pressure = increase in volume}\text{.}$

(d)

Interpretation Introduction

Interpretation:

The given equilibrium system is

  ${\text{CO}}_{\text{2}}{}_{\text{(g)}}{\text{ + Ca(OH)}}_{\text{2(s)}}\rightleftharpoons {\text{CaCO}}_{\text{3(s)}}{\text{ + H}}_{\text{2}}{\text{O}}_{\text{(l)}}{\text{ΔH}}^{\text{°}}\text{= -113 kJ}$

On removal of one-half of the ${\text{CaCO}}_3$, ${\text{CaCO}}_{\text{3}}$ forms more or not has to be given.