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Chapter 13: Q67E (page 758)

What is the pressure of \(BrCl\) in an equilibrium mixture of \(C{l_2}\), \(B{r_2}\), and \(BrCl\) if the pressure of \(C{l_2}\) in the mixture is \(0.115atm\)and the pressure of \(B{r_2}\) in the mixture is \(0.450atm\)?

\(C{l_2}(g) + B{r_2}(g) \rightleftharpoons 2BrCl(g)\)

\({K_P} = 4.7 \times 1{0^{ - 2}}\)

Short Answer

Expert verified

The pressure ofBrCl is 0.049atm

Step by step solution

01

Given information

\(C{l_2}(g) + B{r_2}(g) \rightleftharpoons 2BrCl(g)\)

  1. Value of equilibrium constant \({K_{\rm{P}}} = 4.7 \times 1{0^{ - 2}}\)
  2. The pressure of \(C{l_2}\)in mixture is \(0.115\,atm\)
  3. The pressure of \(B{r_2}\)in mixture is \(0.450\,atm\)
02

Determine the pressure of \(BrCl\)in mixture

\(\begin{array}{c}{K_P} = \frac{{{{\left( {{P_{BrCl}}} \right)}^2}}}{{{P_{C{l_2}}} \times {P_{B{r_2}}}}}\\{\left( {{P_{BrCl}}} \right)^2} = {P_{C{l_2}}} \times {P_{B{r_2}}} \times {K_P}\\{\left( {{P_{BrCl}}} \right)^2} = 4.7 \times {10^{ - 2}} \times 0.115 \times 0.450\\{\left( {{P_{BrCl}}} \right)^2} = 2.43 \times {10^{ - 3}}\end{array}\)

\(\begin{array}{l}\left( {{P_{BrCl}}} \right) = \sqrt {2.43 \times {{10}^{ - 3}}} \\\left( {{P_{BrCl}}} \right) = 0.049\,atm\end{array}\)

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Most popular questions from this chapter

Write the expression of the reaction quotient for the ionization of HOCN in water.

Question: The binding of oxygen by hemoglobin (Hb), giving oxyhemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as

HbO2(aq) + H3 O+(aq) + CO2(g) 鈬� CO2 鈭扝产鈭扝+ + O2(g) + H2 O(l)

(a) Write the equilibrium constant expression for this reaction.

(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxyhemoglobin in the blood passing through the muscle.

The following equation represents a reversible decomposition:

\({\mathbf{CaC}}{{\mathbf{O}}_3}{\text{ }}\left( {\mathbf{s}} \right) \rightleftharpoons {\mathbf{CaO}}\left( {\mathbf{s}} \right){\text{ }} + {\text{ }}{\mathbf{C}}{{\mathbf{O}}_2}{\text{ }}\left( {\mathbf{g}} \right):\)

Under what conditions will decomposition in a closed container proceed to completion so that no \({\bf{CaC}}{{\bf{O}}_3}\) remains?

Nitrogen and oxygen react at high temperatures.

(a) Write the expression for the equilibrium constant \(\left( {{K_c}} \right)\)for the reversible reaction

\(\Delta H = 181kJ\)

(b) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if more \({O_2}\)is added?

(c) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if \({N_2}\)is removed?

(d) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if \(NO\)is added?

(e) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if the temperature of the system is increased?

(g) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if a catalyst is added?

Convert the values of Kc to values of Kp or the values of Kp to values of Kc .

\((a)\,{N_2}\left( g \right) + 3{H_2}\left( g \right)\rightleftharpoons 2N{H_3}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_C} = 0.50\,\,at\,\,400^\circ C\)

\((b){{\rm{H}}_2}(g) + {{\rm{I}}_2}(g)\rightleftharpoons 2HI(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_c} = 50.2\,at\,{448^\circ }{\rm{C}}\)

\((c)N{a_2}{\rm{S}}{{\rm{O}}_4} \cdot 10{{\rm{H}}_2}O(s)\rightleftharpoons N{a_2}{\rm{S}}{{\rm{O}}_4}(s) + 10{{\rm{H}}_2}O(g){K_P} = 4.08 \times {10^{ - 25}}at\,{25^\circ }{\rm{C}}\)

\((d){{\rm{H}}_2}{\rm{O}}(l)\rightleftharpoons {{\rm{H}}_2}{\rm{O}}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_P} = 0.122\,at\,{50^\circ }{\rm{C}}\)
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