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Chapter 13: Q72E (page 759)

Calcium chloride 6−hydrate, \(CaC{l_2}.6{H_2}O\), dehydrates according to the equation

\(CaC{l_2} \times 6{H_2}O(s) \rightleftharpoons CaC{l_2}(s) + 6{H_2}O(g)\)

\({K_P} = 5.09 \times 1{0^{ - 44}}at2{5^o}C\)

What is the pressure of water vapor at equilibrium with a mixture of \(CaC{l_2}.6{H_2}O\)and \(CaC{l_2}\)?

Short Answer

Expert verified

The pressure of water vapor at equilibrium is \(6.09x1{0^{ - 8}}\)atm.

Step by step solution

01

Given information:

\(CaC{l_2}(s),6{H_2}O \rightleftharpoons CaC{l_2} + 6{H_2}O\)
  1. Value of equilibrium constant at \(2{5^0}C\)is \({K_P} = 5.09 \times 1{0^{ - 44}}\)

The value of equilibrium water vapor pressure needs to be calculated

02

Calculate the pressure of water vapor at equilibrium:

\(\begin{array}{*{20}{c}}{{K_p}}&{ = {{\left( {{P_{{H_2}{\rm{O}}}}} \right)}^6}}\\{{P_{{{\rm{H}}_2}{\rm{O}}}}}&{ = \sqrt[6]{{{K_p}}}}\\{}&{ = \sqrt[6]{{5.09 \times {{10}^{ - 44}}}}}\\{}&{}\\{}&{ = 6.09 \times {{10}^{ - 8}}{\rm{atm}}}\end{array}\)

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Most popular questions from this chapter

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

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

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

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

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

Carbon reacts with water vapor at elevated temperatures

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

\({K_c} = 0.2at100{0^o}C\)

What is the concentration of CO in an equilibrium mixture with \(\left[ {{H_2}O} \right] = 0.500M\)at \(100{0^0}C\)?

Write the reaction quotient expression for the ionization of NH3 in water:

Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2produced when a sample of NOCl with a pressure of 10.0 atm comes to equilibrium according to this reaction:

\(2NOCl(g) \rightleftharpoons 2NO(g) + C{l_2}(g)\quad {K_P} = 4.0 \times 1{0^{ - 4}}\)

The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction) in which each system will proceed to leach equilibrium.
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