Chemistry, 05.07.2019 19:10 daniiltemkin20
The equilibrium constant for the reaction agbr(s) picture ag+(aq) + br− (aq) is the solubility product constant, ksp = 7.7 × 10−13 at 25°c. calculate δg for the reaction when [ag+] = 1.0 × 10−2 m and [br-] = 1.0 × 10−3 m. is the reaction spontaneous or nonspontaneous at these concentrations?
Answers: 3
:![K_c=\frac{[Ag^+][Br^-]}{[AgCl]}=\frac{[Ag^+][Br^-]}{1}=[Ag^+][Br^-]](/tpl/images/0055/1226/d9269.png)
![K_{sp}=[Ag^+][Br^-]=K_c=7.7\times 10^{-13}](/tpl/images/0055/1226/964b9.png)
![\Delta G^o=-2.303\times 8.314 J/K mol\times 298 K\times \log[7.7\times 10^{-13}]](/tpl/images/0055/1226/37a54.png)
![[Ag^+] = 1.0\times 10^{-2} M](/tpl/images/0055/1226/88952.png)
and ![[Br^-] = 1.0\times 10^{-3} M](/tpl/images/0055/1226/50b47.png)
![Q=[Ag^+][Br^-]=1.0\times 10^{-2} M\times 1.0\times 10^{-3} M=1.0\times 10^{-5}](/tpl/images/0055/1226/4f48a.png)
![\Delta G=69.117 kJ/mol+(2.303\times 8.314 Joule/mol K\times 298 K\times \log[1.0\times 10^{-5}])](/tpl/images/0055/1226/947e2.png)
.For reaction to non spontaneous reaction: 
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The equilibrium constant for the reaction agbr(s) picture ag+(aq) + br− (aq) is the solubility produ...
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