Equilibrium Tes...

At 1400 K, $$K_c = 2.5 \times 10^{3}$$ for the reaction $$CH_4 (g) + 2H_2S \rightleftharpoons CS_2 (g) + 4H_2 (g)$$. A 10.0 L reaction vessel at 1400 K contains 2.0 mol of $$CH_4$$, 3.0 mol of $$CS_2$$, 3.0 mol of $$H_2$$ and 4.0 mol of $$H_2S$$.The reaction will proceed from right to left to reach equilibrium.

Calculate change in concentration of $${H}^{+}$$ ion in one litre of water,when temperature changes from $$298K$$ to $$310K$$. [Given $${K}_{w}(298)={10}^{-14}, {K}_{w}(310)=2.56\times {10}^{-14}]$$.

What is the $$K_b$$ for $$NH_2$$ group in glycine?

For the reaction $$CO(g) + H_2O \:(g)\rightleftharpoons CO_2 \:(g) + H_2 \:(g)$$ at a given temperature the equilibrium amount of $$CO_2 \:(g)$$ can be increased by :

Reaction $$2BaO_2(s)\rightleftharpoons 2BaO(s) + O_2 \: (g) \: ; \: \Delta H= + ve$$. At equilibrium condition, Pressure of $$O_2$$ is depends on :

Listed in the table are forward and reverse rate constants for the reaction $$2NO (g) \rightleftharpoons N_2 (g) + O_2 (g)$$.

An equimolar solution of $${NaNO_2}$$ and $${HNO_2}$$ can act as a:

The ionization constant of water is related to ionic product as: