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Chapter 13: Q16E (page 751)

Write the mathematical expression for the reaction quotient, \({Q_c}\), for each of the following reactions:

(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 required reaction quotient is \({Q_c} = \frac{{{{\left| {N{H_3}} \right|}^2}}}{{\left( {{{\left. {\;{N_2}||{H_2}} \right|}^3}} \right.}}\)
  2. The required reaction quotient is \({Q_c} = \frac{{\left| {N{O^4}} \right|{H_2}O{O^6}}}{{{{\left| {N{H_3}} \right|}^4}{{\left| {{O_2}} \right|}^3}}}\)
  3. The required reaction quotient is \({Q_c} = \frac{{\left| {{N_2}{O_4}} \right|}}{{{{\left| {N{O_,}} \right|}^2}}}\)
  4. The required reaction quotient is \({Q_c} = \frac{{\left| {C{O^{\\mid {H_2}O}}} \right|}}{{\left| {C{O_2}} \right|\left| {{H_2}} \right|}}\)
  5. The required reaction quotient is \({Q_c} = \left( {N{H_3}} \right)(HCl)\)
  6. The required reaction quotient is \({Q_c} = {\left( {N{O_2}} \right)^4}\left( {{O_2}} \right)\)
  7. The required reaction quotient is \({Q_c} = \frac{1}{{{{\left| {{H_2}} \right|}^2}\left| {{O_2}} \right|}}\)
  8. The required reaction quotient is \({Q_c} = \frac{{|S{|^8}}}{{\left| {{S_8}} \right|}}\)

Step by step solution

01

Definition of reaction quotient

  • Under non-equilibrium conditions, the reaction quotient 'Q' is defined as the ratio of the product of initial product concentrations to the product of initial reactant concentrations.
02

Determine the reaction quotient \({Q_c}\) for  \({N_2}(g) + 3{H_2}(g)  \rightleftharpoons  2N{H_3}(g)\)

(a)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^q}|D{|^d}}}{{|A{|^\mid }|B{|^b}}}\)

So the reaction, \({N_2}(\;g) + 3{H_2}(\;g) \rightleftharpoons 2N{H_3}(\;g)\)

The required reaction quotient is

\({Q_c} = \frac{{{{\left| {N{H_3}} \right|}^2}}}{{|\;N|{{\left| {{H_3}} \right|}^3}}}\)

03

Determine the reaction quotient \({Q_c}\) for \(4N{H_3}(g) + 5{O_2}(g)  \rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

(b)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction,\(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^\mid }|B{|^b}}}\)

So, the reaction \(4N{H_3}(\;g) + 5{O_2}(\;g)\rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

The required reaction quotient is \({Q_c} = \frac{{\left| {N{O^4}} \right|{H_2}O{O^6}}}{{{{\left| {N{H_3}} \right|}^4}{{\left| {{O_2}} \right|}^3}}}\)

04

Determine the reaction quotient \({Q_c}\) for \({N_2}{O_4}(g) \rightleftharpoons 2N{O_2}(g)\)

(c)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^\mid }|B{|^b}}}\)

So, the reaction, \({N_2}{O_4}(\;g) \rightleftharpoons 2N{O_2}(\;g)\)

The required reaction quotient is \({Q_c} = \frac{{\left| {{N_2}{O_4}} \right|}}{{{{\left| {N{O_,}} \right|}^2}}}\)

05

Determine the reaction quotient \({Q_c}\)for \(C{O_2}(g) + {H_2}(g)\rightleftharpoons  CO(g) + {H_2}O(g)\) 

(d) In the case of any reversible response, \({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^{a\mid }}|B{|^b}}}\)

So, the reaction, \(C{O_2}(\;g) + {H_2}(\;g) \rightleftharpoons CO(g) + {H_2}O(g)\)

The required reaction quotient is \({Q_c} = \frac{{\left| {C{O^{\mid {H_2}O}}} \right|}}{{\left| {C{O_2}} \right|\left| {{H_2}} \right|}}\)

06

Determine the reaction quotient \({Q_c}\) for \(N{H_4}Cl(s) \rightleftharpoons N{H_3}(g) + HCl(g)\) 

(e)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^{a\mid }}|B{|^b}}}\)

Furthermore, because the concentration of pure solids and liquids does not fluctuate considerably during the course of a reversible reaction, the concentration term for them is not included in the reaction quotient.

So, the reaction, \(N{H_4}Cl(s) \rightleftharpoons N{H_3}(\;g) + HCl(g)\)

The required reaction quotient is \({Q_c} = \left( {N{H_3}} \right)(HCl)\)

07

Determine the reaction quotient \({Q_c}\)for \(2\;Pb{\left( {N{O_3}} \right)_2}(s) \rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)

(f)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^{a\mid }}|B{|^b}}}\)

Furthermore, because the concentration of pure solids and liquids does not change much during a reversible reaction, the concentration term for them is not included in the reaction quotient.

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

The required reaction quotient is \({Q_c} = {\left( {N{O_2}} \right)^4}\left( {{O_2}} \right)\)

08

Determine the reaction quotient \({Q_c}\) for \(2{H_2}(g) + {O_2}(g) \rightleftharpoons 2{H_2}O(l)\)

(g) In the case of any reversible response, \({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^{a\mid }}|B{|^b}}}\)

So, the reaction \(2{H_2}(\;g) + {O_2}(\;g) \rightleftharpoons 2{H_2}O(l)\)

Furthermore, because the concentration of pure solids and liquids does not change much during a reversible reaction, the concentration term for them is not included in the reaction quotient.

The required reaction quotient is \({Q_c} = \frac{1}{{{{\left| {{H_2}} \right|}^2}\left| {{O_2}} \right|}}\)

09

Determine the reaction quotient \({Q_c}\) for \({S_8}(g) \rightleftharpoons  8\;S(g)\)

(h)

In the case of any reversible response,\({Q_c}\), is the product of all the reactants' concentrations increased to the power of their individual reaction coefficients.

For the form's reversible reaction, \(aA + bB \rightleftharpoons cC + dD\)

\({Q_c} = \frac{{\mid C{)^c}|D{|^d}}}{{|A{|^{a\mid }}|B{|^b}}}\)

So, the reaction, \({S_8}(g) \rightleftharpoons 8\;S(g)\)

The required reaction quotient is \({Q_c} = \frac{{|S{|^8}}}{{\left| {{S_8}} \right|}}\)

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Most popular questions from this chapter

When heated, iodine vapor dissociates according to this equation: I2 (g) 鈬� 2I (g). At 1274K a sample exhibits a partial pressure of I2 of 0.1122 and a partial pressure due to I atoms of 0.1378 atm. Determine the value of the equilibrium constant, Kp for the decomposition at 1274K

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide (\({\rm{S}}{{\rm{O}}_3}\)), from sulfur dioxide (\({\rm{S}}{{\rm{O}}_2}\)), and oxygen (\({{\rm{O}}_2}\)), shown here.

\(2{\text{S}}{{\text{O}}_2}(g) + {{\text{O}}_2}(g) \rightleftharpoons 2{\text{S}}{{\text{O}}_3}(g)\)

At high temperatures, the rate of formation of \({\rm{S}}{{\rm{O}}_3}\)is higher, but the equilibrium amount (concentration or partial pressure) of \({\rm{S}}{{\rm{O}}_3}\) is lower than it would be at lower temperatures.

(a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases?

(b) Is the reaction endothermic or exothermic?

A sample of ammonium chloride was heated in a closed container. NH4 Cl (s)鈬� NH3 (g) + HCl(g)at equilibrium, the pressure of NH3 (g)was found to be 1.75 atm. What is the value of the equilibrium constant, Kp, for the decomposition at this temperature?

How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each?

a. \(2{\rm{N}}{{\rm{H}}_3}(g)\rightleftharpoons {{\rm{N}}_2}(g) + 3{{\rm{H}}_2}(g)\) \({\rm{\Delta }}H = 92{\rm{kJ}}\)

b. \({{\rm{N}}_2}(g) + {{\rm{O}}_2}(g)\rightleftharpoons 2{\rm{NO}}(g)\) \({\rm{\Delta }}H = 181{\rm{kJ}}\)

c. \(2{{\rm{O}}_3}(g)\rightleftharpoons 3{{\rm{O}}_2}(g)\) \({\rm{\Delta }}H = - 285{\rm{kJ}}\)

d.\({\rm{CaO(s) + C}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\rightleftharpoons {\rm{CaC}}{{\rm{O}}_{\rm{3}}}{\rm{(s)}}\) \({\rm{\Delta }}H = - 176{\rm{kJ}}\)

Question: Consider the reaction between \({{\rm{H}}_2}\)and \({{\rm{O}}_2}\)at 100 K\({K_P} = \frac{{{{\left( {{P_{{{\rm{H}}_2}{\rm{O}}}}} \right)}^2}}}{{\left( {{P_{{{\rm{O}}_2}}}} \right){{\left( {{P_{{{\rm{H}}_2}}}} \right)}^2}}} = 1.33 \times {10^{20}}\)

If 0.500 atm of H2 and 0.500 atm of O2are allowed to come to equilibrium at this temperature, what are the partial pressures of the components?

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