Chapter 13: Q66E (page 758)
Calculate the number of moles of \(HI\) that are at equilibrium with \(1.25mol\)of \({H_2}\)and \(1.25\,mol\)of \({I_2}\) in a \(5.00\,L\)flask at \(44{8^0}C\).\({H_2} + {I_2} \rightleftharpoons 2HI\)
\({K_c} = 50.2\,at\,44{8^o}C\)
The number of moles of\(HI\) is \(8.85mol\)
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
(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) \({S_8}(g)\rightleftharpoons 8\;S(g)\)
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium.
(a) \(\begin{aligned}{}2{\rm{N}}{{\rm{H}}_3}(\;{\rm{g}}) \rightleftharpoons {{\rm{N}}_2}(\;{\rm{g}}) + 3{{\rm{H}}_2}(\;{\rm{g}})\;\;\;{K_e} b= 17;\\\;\;\;\left( {{\rm{N}}{{\rm{H}}_3}} \right) = 0.50\,M,\;\left( {{{\rm{N}}_2}} \right) = 0.15\,M,\;\left( {{{\rm{H}}_2}} \right) = 0.12\,M\end{aligned}\)
(b) \(\begin{aligned}{}2{\rm{N}}{{\rm{H}}_3}(\;g) \rightleftharpoons {{\rm{N}}_2}(\;g) + 3{{\rm{H}}_2}(\;g)\;\;\;{K_P} = 6.8 \times {10^4};\\\;\;\;\;{\rm{initial}}\;{\rm{pressures:}}\,{\kern 1pt} {\rm{N}}{{\rm{H}}_3} = 2.00\;{\rm{atm}},\;{\kern 1pt} {\kern 1pt} {{\rm{N}}_2} = 10.00\,{\rm{atm}},\;{{\rm{H}}_2} = 10.00\,{\rm{atm}}\end{aligned}\)
(c) \(\begin{aligned}{}2{\rm{S}}{{\rm{O}}_3}(\;g) \rightleftharpoons 2{\rm{S}}{{\rm{O}}_2}(\;g) + {{\rm{O}}_2}(\;g)\;\;\;{K_c} = 0.230;\\\;{\kern 1pt} {\kern 1pt} {\kern 1pt} \;\left( {{\rm{S}}{{\rm{O}}_3}} \right) = 2.00\,M,\;\left( {{\rm{S}}{{\rm{O}}_2}} \right) = 2.00\,M,\;\left( {{{\rm{O}}_2}} \right) = 2.00\,M\end{aligned}\)
(d) \(\begin{aligned}{}2{\rm{S}}{{\rm{O}}_3}(\;g) \rightleftharpoons 2{\rm{S}}{{\rm{O}}_2}(\;g) + {{\rm{O}}_2}(\;g)\;\;\;{K_p} = 6.5\;{\rm{atm}};\\\;\;\;\;{\rm{initial}}\;{\rm{pressures:}}\;{\rm{S}}{{\rm{O}}_2} = 1.00\;{\rm{atm}},\;{{\rm{O}}_2} = 1.130\;{\rm{atm}},\;{\rm{S}}{{\rm{O}}_3} = 0\;{\rm{atm}}\end{aligned}\)
(e) \(\begin{aligned}{}2{\rm{NO}}(g) + {\rm{C}}{{\rm{l}}_2}(g) \rightleftharpoons 2{\rm{NOCl}}(g)\;\;\;{K_P} = 2.5 \times {10^3};\\\;\;\;\;{\rm{initial}}\;{\rm{pressures:}}\;{\rm{NO}} = 1.00\;{\rm{atm}},{\rm{C}}{{\rm{l}}_2} = 1.00\;{\rm{atm}},\;{\rm{NOCl}} = 0\;{\rm{atm}}\end{aligned}\)
(f) \(\begin{aligned}{}{{\rm{N}}_2}(\;g) + {{\rm{O}}_2}(\;g) \rightleftharpoons 2{\rm{NO}}(g)\;\;\;{K_c} = 0.050;\\\;\;\;\;\;\left( {{{\rm{N}}_2}} \right) = 0.100M,\;\left( {{{\rm{O}}_2}} \right) = 0.200M,\;({\rm{NO}}) = 1.00M\end{aligned}\)
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?
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 \(4.12\)\( \times 1{0^{ - 1}}MN{H_3}\)
What do you think about this solution?
We value your feedback to improve our textbook solutions.
