Question: For reaction $Ag_{2}O(s) \rightarrow 2Ag(s) + \frac{1}{2}O_{2}(g)$ the value of \(\Delta H = 30.56...

Question

For reaction $Ag_{2}O(s) \rightarrow 2Ag(s) + \frac{1}{2}O_{2}(g)$ the value of $\Delta H = 30.56kJmol^{- 1}$ and $\Delta S = 0.066kJmol^{- 1}K^{- 1}.$

Temperature at which free energy change for reaction will be zero is

Answer 1

Solution

$\Delta G = \Delta H - T\Delta S$

$\Delta H = 30.56kJmol^{- 1}$ ; $\Delta S = 0.066kJmol^{- 1}K^{- 1}$ ; $\Delta G = 0$ at equilibrium; $T = ?$

$\therefore\Delta H = T\Delta S$ or $30.56 = T \times 0.066$

$T = 463K$

Question: For reaction \(Ag_{2}O(s) \rightarrow 2Ag(s) + \frac{1}{2}O_{2}(g)\) the value of \(\Delta H = 30.56...

Solution