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Chapter 13: Q68E (page 758)

What is the pressure of \(C{O_2}\)in a mixture at equilibrium that contains \(0.50atm\)\({H_2}\), \(2.0atm\)of \({H_2}O\), and \(1.0atm\)of \(CO\) at \(99{0^0}C\)?

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

\({K_P} = 1.6\,at\, 99{0^o}C\)

Short Answer

Expert verified

The pressure of CO2is 2.5atm

Step by step solution

01

Given information

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

  1. Value of equilibrium constant \({K_{\rm{P}}} = 1.6\)
  2. The pressure of \({H_2}\)in mixture is \(0.50\,atm\)
  3. The pressure of \({{\rm{H}}_{\rm{2}}}{\rm{O}}\)in mixture is \(2.0atm\)
02

Determine the pressure of \(C{O_2}\):

\(\begin{array}{*{20}{c}}{{K_p}}&{ = \frac{{\left[ {{{\rm{H}}_2}{\rm{O}}} \right] \times [{\rm{CO}}]}}{{\left[ {{{\rm{H}}_2}} \right] \times \left[ {{\rm{CO}}{{\rm{O}}_2}} \right]}}}\\{\left[ {{\rm{C}}{{\rm{O}}_2}} \right]}&{ = \frac{{\left[ {{{\rm{H}}_2}{\rm{O}}} \right] \times [{\rm{CO}}]}}{{\left[ {{{\rm{H}}_2}} \right] \times {{\rm{K}}_p}}}}\\{}&{ = \frac{{2.0 \times 1.0}}{{0.50 \times 1.6}}}\\{}&{ = 2.5{\rm{atm}}}\end{array}\)

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Most popular questions from this chapter

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) ⇌ 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 \(4.12\)\( \times 1{0^{ - 1}}MN{H_3}\)

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

\((a)\,C{l_2}\left( g \right) + B{r_2}\left( g \right)\rightleftharpoons 2BrCl(g)\,\,\,{K_C} = 4.7 \times {10^{ - 2}}\,at\,25^\circ C\)

\((b)2{\rm{S}}{{\rm{O}}_2}(g) + {{\rm{O}}_2}(g)\rightleftharpoons 2{\rm{S}}{{\rm{O}}_3}(g){K_P} = 48.2 at {500^\circ} {\rm{C}}\)

\((c){\rm{CaC}}{{\rm{l}}_2} \cdot 6{{\rm{H}}_2}{\rm{O}}(s)\rightleftharpoons {\rm{CaC}}{{\rm{l}}_2}(s) + 6{{\rm{H}}_2}{\rm{O}}(g){K_P} = 5.09 \times {10^{ - 44}}at{25^\circ }{\rm{C}}\)

\((d){{\rm{H}}_2}{\rm{O}}(l)\rightleftharpoons {{\rm{H}}_2}{\rm{O}}(g)\,{K_P} = 0.196\,at\,{60^\circ }{\rm{C}}\)

Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.

Analysis of the gases in a sealed reaction vessel containing \(N{H_3}\), \({N_2}\), and \({H_2}\) at equilibrium at \(40{0^0}C\) established the concentration of \({N_2}\) to be \(1.2M\) and the concentration of \({H_2}\) to be \(0.24M\).

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

\({K_c} = 0.50\,at\,40{0^o}C\)

Calculate the equilibrium molar concentration of \(N{H_3}\).

Cobalt metal can be prepared by reducing cobalt (II) oxide with carbon monoxide.

\(CoO(s) + CO(g) \rightleftharpoons Co(s) + C{O_2}(g)\)

\({K_c} = 4.90 \times 1{0^2}at55{0^o}C\)

What concentration of \(CO\) remains in an equilibrium mixture with \(\left[ {C{O_2}} \right] = 0.100M\)

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