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Chapter 13: Q31 E (page 752)

The following equation represents a reversible decomposition:

\({\mathbf{CaC}}{{\mathbf{O}}_3}{\text{ }}\left( {\mathbf{s}} \right) \rightleftharpoons {\mathbf{CaO}}\left( {\mathbf{s}} \right){\text{ }} + {\text{ }}{\mathbf{C}}{{\mathbf{O}}_2}{\text{ }}\left( {\mathbf{g}} \right):\)

Under what conditions will decomposition in a closed container proceed to completion so that no \({\bf{CaC}}{{\bf{O}}_3}\) remains?

Short Answer

Expert verified

The amount of \({\rm{CaC}}{{\rm{O}}_3}\) Will not be able to generate the required \({{\rm{P}}_{\rm{C}}}{{\rm{O}}_2}\) to establish an equilibrium.

Step by step solution

01

Using the Le Châtelier's Principle:

When\({\rm{CaC}}{{\rm{O}}_3}\)decomposes,\({{\rm{P}}_{\rm{C}}}{{\rm{O}}_2}\) becomes less than\({{\rm{K}}_p}\) making the amount of\({\rm{CaC}}{{\rm{O}}_3}\)lesser.

Meaning, the amount of\({\rm{CaC}}{{\rm{O}}_3}\)Will not be able to generate the required\({{\rm{P}}_{\rm{C}}}{{\rm{O}}_2}\) to establish an equilibrium.

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Most popular questions from this chapter

Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.

What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5 (l)⇌C2 H5OC2H5 (g) at 25 °C.

(Vapor pressure was described in the previous chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)

How will an increase in temperature affect each of the following equilibrium? How will a decrease in the volume of the reaction vessel affect each?

\(\begin{gathered} (a)2{H_2}O(g) \rightleftharpoons 2{H_2}(g) + {O_2}(g) \hfill \\ \Delta H = 484kJ \hfill \\ (b){N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g) \hfill \\ \Delta H = - 92.2kJ \hfill \\ (c)2Br(g) \rightleftharpoons B{r_2}(g) \hfill \\ \Delta H = - 224kJ \hfill \\ (d){H_2}(g) + {I_2}(s) \rightleftharpoons 2HI(g) \hfill \\ \Delta H = 53kJ \hfill \\ \end{gathered}\)

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?

Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?

\({\rm{S}}{{\rm{O}}_2}{\rm{C}}{{\rm{l}}_2}(g)\rightleftharpoons {\rm{S}}{{\rm{O}}_2}(g) + {\rm{C}}{{\rm{l}}_2}(g)\)

\(\left( {{\rm{S}}{{\rm{O}}_2}{\rm{C}}{{\rm{l}}_2}} \right) = 0.12\;{\rm{M}},\;\left( {{\rm{C}}{{\rm{l}}_2}} \right) = 0.16\;{\rm{M and }}\left( {{\rm{S}}{{\rm{O}}_2}} \right) = 0.050\;{\rm{M}}.\;{K_c}\) for the reaction is 0.078.
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