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For the decomposition of $Ag_2O$ at 298 K. $Ag_2O (s) \longrightarrow 2Ag(s) + \frac{1}{2} O_2(g) \Delta G^\circ$ = 11.21 kJ which of the following statement is true?


(a) It cannot be made spontaneous without increasing the temperature.
(b) It can be made spontaneous by decreasing the pressure at 298 K.
(c) It can be made spontaneous by increasing the pressure at 298 K.
(d) None of the above

Can you answer this question?
 
 

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Answer: It can be made spontaneous by decreasing the pressure at 298 K.
For the reaction to be spontaneous, $\Delta G = -ve$
At equilibrium, $\Delta G =0$
$\Delta G = \Delta G^\circ - 2.303$ RT log $(p_{O_2})^{\frac{1}{2}}$
$\Rightarrow 0 = +11210 - 2.303\times (8.31) \times 298$ log $(p_{O_2})^{\frac{1}{2}}$
Solving $(p_{O_2})$ = 0.000116 atm = 0.089 torr
Therefore, at a pressure of less than 0.089 torr, the reaction is spontaneous.
answered Feb 28, 2014 by mosymeow_1
edited Apr 2, 2014 by pradeesh.chinnasamy_1
 

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