Chapter 13: Q13E (page 750)
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%.
Is \({K_c} > 1,\; < 1\), or \( \approx 1\) for a titration reaction?
As titration reactions are rapid and yield is almost 100%, so \({K_c} > 1.\)
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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.
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?
How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each?
a. \(2{\rm{N}}{{\rm{H}}_3}(g)\rightleftharpoons {{\rm{N}}_2}(g) + 3{{\rm{H}}_2}(g)\) \({\rm{\Delta }}H = 92{\rm{kJ}}\)
b. \({{\rm{N}}_2}(g) + {{\rm{O}}_2}(g)\rightleftharpoons 2{\rm{NO}}(g)\) \({\rm{\Delta }}H = 181{\rm{kJ}}\)
c. \(2{{\rm{O}}_3}(g)\rightleftharpoons 3{{\rm{O}}_2}(g)\) \({\rm{\Delta }}H = - 285{\rm{kJ}}\)
d.\({\rm{CaO(s) + C}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\rightleftharpoons {\rm{CaC}}{{\rm{O}}_{\rm{3}}}{\rm{(s)}}\) \({\rm{\Delta }}H = - 176{\rm{kJ}}\)
For which of the reactions in Exercise 13.16 does \({K_c}\) (calculated using concentrations) equal \({K_p}\)(calculated using pressures)?
(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) \({S_8}(g)\rightleftharpoons 8\;S(g)\)
Question: Calculate the number of grams of HI that are at equilibrium with 1.25 mol of H2 and 63.5 g of iodine at 448°C.
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