Chapter 13: Q51E (page 755)
Question: A reaction is represented by this equation: \({K_c} = 1 \times 1{0^3}\)
(a) Write the mathematical expression for the equilibrium constant.
The value of equilibrium constant\(({\rm{A}}) = 0.1{\rm{M}}({\rm{B}}) = 0.1{\rm{M}}({\rm{C}}) = 1{\rm{M}}\)
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Calculate the equilibrium concentrations of NO, O2, and NO2 in a mixture at 250 °C that results from the reaction of 0.20 M NO and 0.10 M O2. (Hint: K is large; assume the reaction goes to completion then comes back to equilibrium.)
\(2NO(g) + {O_2}(g) \rightleftharpoons 2N{O_2}(g)\quad {K_c} = 2.3 \times 1{0^5}\;at\;25{0^o}C\)
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.
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 \(100{0^0}C\)?
Question: Antimony pentachloride decomposes according to this equation:
An equilibrium mixture in a 5.00-L flask at 4480C contains 3.85 g of \({\rm{SbC}}{{\rm{l}}_5}\),9.14 g of \({\rm{SbC}}{{\rm{l}}_3}\)and 2.84 g of \({\rm{C}}{{\rm{l}}_2}\).How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?
Write the mathematical expression for the reaction quotient, \({Q_c}\), for each of the following reactions:
(a) \({N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)\)
(b) \(4N{H_3}(g) + 5{O_2}(g) \rightleftharpoons 4NO(g) + 6{H_2}O(g)\)
(c) \({N_2}{O_4}(g) \rightleftharpoons 2N{O_2}(g)\)
(d) \(C{O_2}(g) + {H_2}(g) \rightleftharpoons CO(g) + {H_2}O(g)\)
(e) \(N{H_4}Cl(s) \rightleftharpoons N{H_3}(g) + HCl(g)\)
(f) \(2\;Pb{\left( {N{O_3}} \right)_2}(s) \rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)
(g) \(2{H_2}(g) + {O_2}(g) \rightleftharpoons 2{H_2}O(l)\)
(h) \({S_8}(g) \rightleftharpoons 8\;S(g)\)
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