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Chapter 13: Q22E (page 752)

Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?

(a) \({N_2}(g) + 3{H_2}(g)\rightleftharpoons 2N{H_3}(g)\)

(b) \(4N{H_3}(g) + 5{O_2}(g)\rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

(c) \({N_2}{O_4}(g)\rightleftharpoons 2N{O_2}(g)\)

(d) \(C{O_2}(g) + {H_2}(g)\rightleftharpoons CO(g) + {H_2}O(g)\)

(e) \(N{H_4}Cl(s)\rightleftharpoons N{H_3}(g) + HCl(g)\)

(f) \(2\;Pb{\left( {N{O_3}} \right)_2}(s)\rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)

(g) \(2{H_2}(g) + {O_2}(g)\rightleftharpoons 2{H_2}O(l)\)

(h) \({S_8}(g)\rightleftharpoons 8\;S(g)\)

Short Answer

Expert verified
  1. The system is Homogenous.
  2. The system is Homogenous.
  3. The system is Homogenous.
  4. The system is homogenous.
  5. The system is Heterogenous.
  6. The system is heterogeneous.
  7. The system is Heterogenous.
  8. The system is homogenous.

Step by step solution

01

Definition of equilibria

When reactants and products are in different phases in a chemical reaction, heterogeneous equilibria is obtained, and when they are in the same phase, homogeneous equilibria is obtained.

02

Find the system of equilibriafor part (a)

a.

The given system is:

\({{\rm{N}}_2}(\;{\rm{g}}) + 3{{\rm{H}}_2}(\;{\rm{g}})\rightleftharpoons 2{\rm{N}}{{\rm{H}}_3}(\;{\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is in homogenous equilibria.

03

Determine the system of equilibriafor part (b)

b.

The given system is:

\(4{\rm{N}}{{\rm{H}}_3}(\;{\rm{g}}) + 5{{\rm{O}}_2}(\;{\rm{g}})\rightleftharpoons 4{\rm{NO}}({\rm{g}}) + 6{{\rm{H}}_2}(\;{\rm{g}})\)

Here both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is in homogenous equilibria.

04

Detect the system of equilibriafor part (c)

C.

The given system is:

\({{\rm{N}}_2}{{\rm{O}}_4}(\;{\rm{g}})\rightleftharpoons2{\rm{N}}{{\rm{O}}_2}(\;{\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is in homogenous equilibria.

05

Discover the system of equilibriafor part (d)

d.

The given system is:

\({\rm{C}}{{\rm{O}}_2}(\;{\rm{g}}) + {{\rm{H}}_2}(\;{\rm{g}})\rightleftharpoons {\rm{CO}}({\rm{g}}) + {{\rm{H}}_2}{\rm{O}}({\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is in homogenous equilibria.

06

Determine the system of equilibriafor part (e)

e.

The given system is:

\({\rm{N}}{{\rm{H}}_4}{\rm{Cl}}({\rm{s}}) \rightleftharpoons {\rm{N}}{{\rm{H}}_3}(\;{\rm{g}}) + {\rm{HCl}}({\rm{g}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

07

Detect the system of equilibriafor part (f)

F.

The given system is:

\(2\;{\rm{Pb}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(\;{\rm{s}})\rightleftharpoons 2{\rm{PbO}}({\rm{s}}) + 4{\rm{N}}{{\rm{O}}_2}(\;{\rm{g}}) + {{\rm{O}}_2}(\;{\rm{g}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

08

Find the system of equilibriafor part (g)

g.

The given system is as follows:

\(2{{\rm{H}}_2}(\;{\rm{g}}) + {{\rm{O}}_2}(\;{\rm{g}})\rightleftharpoons 2{{\rm{H}}_2}{\rm{O}}({\rm{l}})\)

The phases of reactant and product are different, i.e. solid and gas. So, the system is in heterogeneous equilibrium.

09

Discover the system of equilibriafor part (h)

h.

The given system is:

\({{\rm{S}}_8}(\;{\rm{g}})\rightleftharpoons 8\;{{\rm{S}}_8}(\;{\rm{g}})\)

Both reactant and product are in same phase, i.e. in the gaseous phase. So, the system is in homogenous equilibria.

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Most popular questions from this chapter

Question : A 0.010Msolution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 掳C. A 0.010Msolution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions.

(a) Which acid has the larger equilibrium constant for ionization

HA[HA(aq) 鈬� A鈭�(aq) + H+(aq)]or HB[HB(aq) 鈬� H+(aq) + B鈭�(aq)]?

(b) What are the equilibrium constants for the ionization of these acids?

(Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB), the conjugate base (A鈭� or B鈭�), and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)

Question:What is the value of the equilibrium constant at \(50{0^o}C\) for the formation of \(N{H_3}\)according to the following equation? N2(g) + 3H2(g) 鈬� 2NH3(g)

An equilibrium mixture of \(N{H_3}(g)\) \({H_2}(g)\) and \({N_2}(g)\) at \(50{0^o}C\) was found to contain\(1.35M{H_2},1.15M{N_2}\)and \(4.12\)\( \times 1{0^{ - 1}}MN{H_3}\)

What are all concentrations after a mixture that contains \(\left[ {{{\bf{H}}_{\bf{2}}}{\bf{O}}} \right] = {\bf{1}}.{\bf{00Mand}}\left[ {{\bf{C}}{{\bf{l}}_{\bf{2}}}{\bf{O}}} \right] = {\bf{1}}.{\bf{00M}}\) comes to equilibrium at \({\bf{25}}^\circ {\bf{C}}\)?

\({{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}(g) + {\mathbf{C}}{{\mathbf{l}}_{\mathbf{2}}}{\mathbf{O}}(g) \rightleftharpoons {\mathbf{2HOCl}}(g);\;{\mathbf{Kc}} = {\mathbf{0}}.{\mathbf{0900}}\)

Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.

Question: The density of trifluoroacetic acid vapor was determined at 118.1 掳C and 468.5 torr, and found to be 2.784 g/L.

CalculateKcfor the association of the acid.
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