Question

Choose the disproportionation reaction among the following redox reaction


a) 3Mg(s) + N2(g) ---> Mg3N2(s)

b) P4(s)+3 NaOH+3H2O---> PH3(g)+3NaH2PO2(aq)

c) CL2(g)+2KI(aq)---> 2KCL(aq)+I2

d)Cr2O3(s)+ 2AL(s) ---> AL2O3(s) + 2Cr(s)
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Answer 1

Answer:

sorry don't know

Explanation:

sorry don't know

Answer 2

Answer:

A redox reaction, the species is simultaneously oxidized and reduced to form at least two different products is known as disproportionation redox reaction.

disproportionation reaction can be represented by , 2A ⇒A' + A" , Where A, A' and A" are different chemical species.

Answer :- option (b) 

Explanation :- P₄ ------>PH₃ + NaH₂PO₂ 

Here you can see oxidation state of P is different in all three molecules.

oxidation state of P in P₄ = 0

oxidation state of P in PH₃ = -3 

oxidation state of P in NaH₂PO₂ = +5 

Also P is oxidized as well as reduced in same reaction.

So, it is disproportionation redox reaction.