For a reaction,
4M(s) + nO₂(g) $$ \to $$ 2M₂O_n(s)
the free energy change is plotted as a function of temperature. The temperature below which the oxide is stable could be inferred from the plot as the point at which :

For the given cell :

Cu(s) | Cu²⁺(C₁M) || Cu²⁺(C₂M) | Cu(s)

change in Gibbs energy ($$\Delta $$G) is negative, if :

A set of solutions is prepared using 180 g of water as a solvent and 10 g of different nonvolatile solutes A, B and C. The relative lowering of vapour pressure in the presence of these solutes are in the order :

[Given, molar mass of A = 100 g mol^–1; B = 200 g mol^–1; C = 10,000 g mol^–1]

The value of K_C is 64 at 800 K for the reaction

N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

The value of K_C for the following reaction is :

NH₃(g) ⇌ $${1 \over 2}$$N₂(g) + $${3 \over 2}$$H₂(g)