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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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Question:At 1 atm and \(2{5^o}C,N{O_2}\) with an initial concentration of \(1.00M\;is\;3.3 \times 1{0^{ - 3}}\% \)decomposed into \(NO\;and\;{O_2}\). Calculate the value of the equilibrium constant for the reaction. \(2N{O_2}(g) \rightleftharpoons 2NO(g) + {O_2}(g)\)
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?
\(\begin{gathered} (a)2{H_2}O(g) \rightleftharpoons 2{H_2}(g) + {O_2}(g) \hfill \\ \Delta H = 484kJ \hfill \\ (b){N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g) \hfill \\ \Delta H = - 92.2kJ \hfill \\ (c)2Br(g) \rightleftharpoons B{r_2}(g) \hfill \\ \Delta H = - 224kJ \hfill \\ (d){H_2}(g) + {I_2}(s) \rightleftharpoons 2HI(g) \hfill \\ \Delta H = 53kJ \hfill \\ \end{gathered}\)
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?
\(P\left( {{\rm{N}}{{\rm{H}}_3}} \right) = 93\;{\rm{atm}},\;P\left( {\;{{\rm{N}}_2}} \right) = 48\;{\rm{atm}},\;{\rm{and}}\;P\left( {{{\rm{H}}_2}} \right) = 52\)
Write the mathematical expression for the reaction quotient\({Q_C}\), for each of the following reactions:
(a) \(C{H_4}(g) + C{l_2} \rightleftharpoons C{H_3}CI(g) + HCI(g)\)
(b) \({N_2}(g) + {O_2}(g) \rightleftharpoons 2NO(g)\)
(c) \(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)
(d) \(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)
(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons {P_4}{O_{10}}(s)\)
(f) \(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)
(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)
(h) \(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)
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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