1. What is the equivalent weight of white phosphorus () in the following disproportionation reaction — Electrochemistry Chemistry Question
Question
1. What is the equivalent weight of white phosphorus ($P_4$) in the following disproportionation reaction? $P_4 + 3OH^- + 3H_2O \rightarrow PH_3 + 3H_2PO_2^-$ (where M = molar mass of $P_4$)
Answer: B
💡 Solution & Explanation
In this reaction, $P_4$ (0) oxidises to $H_2PO_2^-$ (+1) losing 4 electrons ($n_1=4$) and reduces to $PH_3$ (-3) gaining 12 electrons ($n_2=12$). The net n-factor is $\frac{n_1 \times n_2}{n_1 + n_2} = \frac{48}{16} = 3$. Hence, Equivalent weight = M/3.
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