Question

Consider the following statements:

(I) An increase in pressure (caused by decrease in volume) at equilibrium results in increase in molar concentration of each gaseous substance involved.

(II) An increase in pressure (caused by decrease in volume) at equilibrium results in increase in no. of moles of each gaseous substance involved.

(III) For the reaction $A\left(s\right)\rightleftharpoons B\left(g\right)+C\left(g\right)$ at constant temperature, total pressure at equilibrium (of $B\left(g\right)$ & $C\left(g\right)$) is not affected by changing the volume of container.

(IV) $H_{2}O\left(l\right)\rightleftharpoons H_{2}O\left(g\right)$ on temperature increase, $K_p$ of this reaction is increased.

Tick the correct statement(s)

• A. (I)
• B. (II)
• C. (III)
• D. (IV)

Answer 1

Answer: (A), (C), (D)

(III)
(IV)
(I)

(I) : $P\propto \frac{n}{V}$

on $P\uparrow \frac{n}{V}\uparrow$

(II) : $P\uparrow$ on, equation shifts in a direction in which no. of moles of gases $\downarrow$

(III) : $K_P=\left(P_B\right)\left(P_C\right)$ (constant at constant temp)

(IV) : $H_{2}O\left(\ell \right)\rightleftharpoons H_{2}O\left(g\right)$ $△H=+ve$

on $T\uparrow$ forward reaction.