The theoretical vapour density of is . When heated, it dissociates as and the observed vapour densit — Chemical Equilibrium Chemistry Question
Question
The theoretical vapour density of $PCl_5$ is $104.16$. When heated, it dissociates as $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$ and the observed vapour density reduces to $62$. What is the degree of dissociation of $PCl_5$?
Answer: A
💡 Solution & Explanation
For $PCl_5 \rightleftharpoons PCl_3 + Cl_2$, $n = 2$. Using $\alpha = (D - d) / ((n - 1)d)$, where $D = 104.16$ and $d = 62$. $\alpha = (104.16 - 62) / 62 = 42.16 / 62 \approx 0.68$, or $68\%$.
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