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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

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

CalculateKcfor the association of the acid.

For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%.

Is \({K_c} > 1,\; < 1\), or \( \approx 1\) for a titration reaction?

For which of the reactions in Exercise 13.15 does\({K_c}\)(calculated using concentrations) equal\({K_p}\)(calculated using pressures)?

(a) \(C{H_4}(g) + C{l_2} \rightleftharpoons C{H_3}CI(g) + HCI(g)\)

(b) \({N_2}(g) + {O_2}(g)\rightleftharpoons 2NO(g)\)

(c) \(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)

(d) \(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)

(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons{P_4}{O_{10}}(s)\)

(f) \(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)

(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)

(h)\(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)

Question: \(\;A\;0.72 - mol\)sample of \(PC{l_5}\)is put into a \(1.00 - L\) vessel and heated. At equilibrium, the vessel contains \(0.40mol\) of \(PC{l_3}(g)\) and \(0.40mol\;of\;C{l_2}(g)\). Calculate the value of the equilibrium constant for the decomposition of \(PC{l_5}\;to\;\)\(PC{l_3}\;and\;C{l_2}\)at this temperature.

Question:At 1 atm and \(2{5^o}C,N{O_2}\) with an initial concentration of \(1.00M\;is\;3.3 \times 1{0^{ - 3}}\% \)decomposed into \(NO\;and\;{O_2}\). Calculate the value of the equilibrium constant for the reaction. \(2N{O_2}(g) \rightleftharpoons 2NO(g) + {O_2}(g)\)
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