MCQ
For the reaction $PC{l_5}_{(g)}$ $\rightleftharpoons$ $PC{l_3}_{(g)} + C{l_2}_{(g)}$
- A${K_p} = {K_c}$
- B${K_p} = {K_c}{(RT)^{ - 1}}$
- ✓${K_p} = {K_c}(RT)$
- D${K_p} = {K_c}{(RT)^2}$
${K_p} = {K_c}(RT)$
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${H_2}(g) + {I_2}(g) \rightleftharpoons 2HI(g)$
is $32$ at a given temperature. The equilibrium concentrations of $I_2$ and $HI$ are $0.5 \times 10^{-3}\, M$ and $8 \times 10^{-3}\, M$ respectively. the equilibrium concentration of $H_2$ is
(Atomic masses of $\mathrm{Ag}$ and $\mathrm{Cl}$ are $107.87$ and $35.5$ respectively)
$(I)$ ${H_2}(g) + \frac{1}{2}{O_2}(g) \to {H_2}O(l);$
$\Delta {H^o_{298\,K}} = - 285.9\,kJ\,mo{l^{ - 1}}$
$(II)$ ${H_2}(g) + \frac{1}{2}{O_2}(g) \to {H_2}O(g);$
$\Delta {H^o_{298\,K}} = - 241.8\,kJ\,mo{l^{ - 1}}$
The molar enthalpy of vapourisation of water will be.....$kJ\,mol^{-1}$