dissociates into and . The theoretical vapour density of is strictly . If at a specific equilibrium — Chemical Equilibrium Chemistry Question
Question
$PCl_5(g)$ dissociates into $PCl_3(g)$ and $Cl_2(g)$. The theoretical vapour density of $PCl_5$ is strictly $104.25$. If at a specific equilibrium temperature, the degree of dissociation $\alpha$ is found to be exactly $0.5$, calculate the numerical value of $(10 \times d)$, where $d$ is the observed vapour density of the mixture.
Answer: 695
💡 Solution & Explanation
For $PCl_5 \rightleftharpoons PCl_3 + Cl_2$, the value of $n = 2$. The formula relating densities is $d = \frac{D}{1 + (n - 1)\alpha} = \frac{D}{1 + \alpha}$. Given $D = 104.25$ and $\alpha = 0.5$, we have $d = \frac{104.25}{1 + 0.5} = \frac{104.25}{1.5} = 69.5$. The question asks for $10 \times d$, which is $10 \times 69.5 = 695$.
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