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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: 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.

Question:Calculate the value of the equilibrium constant \({K_P}\) for the reaction \(2NO(g) + C{l_2}(g) \rightleftharpoons 2NOCl(g)\) from these equilibrium pressures: NO, \(0.050atm;C{l_2},0.30atm;NOCl,1.2atm\)

The following reaction has \({K_P} = 4.50 \times {10^{ - 5}}\) at \(720\;{\rm{K}}\).

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

If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium?

\(P\left( {{\rm{N}}{{\rm{H}}_3}} \right) = 93\;{\rm{atm}},\;P\left( {\;{{\rm{N}}_2}} \right) = 48\;{\rm{atm}},\;{\rm{and}}\;P\left( {{{\rm{H}}_2}} \right) = 52\)

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?

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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