Equilibrium Tes...

The number of hydronium ions in $$1 ml$$ of an aqueous solution of $$pH$$ $$12.0$$ at $$25^{\circ}C$$ is

$$pH$$ of $$0.01 M - (NH_{4})_{2}SO_{4})$$ and $$0.02 M - NH_{4}OH$$ buffer ($$pK_{a}$$ of $$NH_{4}^{+} = 9.26$$) is

For the reaction : $$ PCl_5(g) \leftrightharpoons PCl_3(g) + Cl_2(g) $$, if initial moles of $$ PCl_5 $$ is 'x', a is the degree of dissociation and P is total pressure at equilibrium , then $$ P_{PCl_3 } . P^{-1} $$ is equal to

$$ K_p $$ for the reaction : $$ N_2O_4(g) \leftrightharpoons NO_2 $$ is 640 mm at 775 K. The percentage dissociation of $$ N_2O_4$$ at equilibrium pressure of 160 m is:

$$pH$$ of water is $$7.0$$ at $$25^{\circ}C$$. If water is heated to $$70^{\circ}C$$, the

Nitrogen dioxide, $$NO_{2}$$, exists in equilibrium with dinitrogen tetroxide, $$N_{2}O_{4}$$.
$$2NO_{2}(g)\rightleftharpoons N_{2}O_{4}(g)\ \triangle H = -57kJ\ mol^{-1}$$
Which conditions give the greatest percentage of $$N_{2}O_{4}(g)$$ at equilibrium?

For the reaction : $$ XY_2 (g) \leftrightharpoons XY(g) + Y (g) $$ the reaction is started with initial pressure of $$ XY_2 $$, $$600$$ mmHg. The total pressure for gases at equilibrium is 800 mmHg. Assuming volume and temperature of the system remains constant, the value of the $$ K_p $$ is

The reaction between sulfur dioxide and oxygen is reversible.
$$2SO_2+O_2\rightleftharpoons 2SO_3$$
$$\Delta H^{\bigoplus}=-196$$ kJ $$mol^{-1}$$
Which conditions of pressure and temperature favour the reverse reaction?

Saccharin ($$K_{a} = 2 \times 10^{-12}$$) is a weak acid represented by formula, $$HSac$$. A $$4 \times 10^{-4}$$ mole amount of saccharin is dissolved in $$200 ml$$ water of $$pH$$, $$3.0$$. Assuming no change in volume, the concentration of $$Sac^{-1}$$ ions in the resulting solution at equilibrium is

For the equilibrium $$PCl_5 \rightleftharpoons PCl_3 + Cl_2$$, $$K_p =\dfrac{\alpha^2}{(1 - \alpha) V}$$, temperature remaining constant,