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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

When heated, iodine vapor dissociates according to this equation: I2 (g) ⇌ 2I (g). At 1274K a sample exhibits a partial pressure of I2 of 0.1122 and a partial pressure due to I atoms of 0.1378 atm. Determine the value of the equilibrium constant, Kp for the decomposition at 1274K

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

Assume that the change in pressure of \({H_2}S\) is small enough to be neglected in the following problem.(a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm.

\(2{H_2}S(g) \rightleftharpoons 2{H_2}(g) + {S_2}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_p} = 2.2 \times {10^{( - 6)}}\)

(b) Show that the change is small enough to be neglected.

Question: What is the minimum mass of CaCO3 required to establish equilibrium at a certain temperature in a 6.50-L container if the equilibrium constant (Kc) is 0.050 for the decomposition reaction of CaCO3 at that temperature?

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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