The degree of dissociation $(\alpha )$ of $PCl_5$ obeying the equilibrium; is $PC{l_5}\, \rightleftharpoons \,PC{l_3}\, + \,C{l_2}$ related to the pressure at equlibrium by
The degree of dissociation $(\alpha )$ of $PCl_5$ obeying the equilibrium; is $PC{l_5}\, \rightleftharpoons \,PC{l_3}\, + \,C{l_2}$ related to the pressure at equlibrium by
- A
$\alpha \, \propto \,P$
- B
$\alpha \, \propto \,\frac{1}{{\sqrt P }}$
- C
$\alpha \, \propto \,\frac{1}{{{P^2}}}$
- D
$\alpha \, \propto \,\frac{1}{{{P^4}}}$
Similar Questions
Which oxychloride has maximum $pH$
Which oxychloride has maximum $pH$
A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be
The degree of ionization of a $0.1 \,M$ bromoacetic acid solution is $0.132$ Calculate the $pH$ of the solution and the $p K_{ a }$ of bromoacetic acid.
The degree of ionization of a $0.1 \,M$ bromoacetic acid solution is $0.132$ Calculate the $pH$ of the solution and the $p K_{ a }$ of bromoacetic acid.
$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be
$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be
At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be
At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be