A 2.5 mol of hydrazine N2H4 loses 25 mole of electrons is being converted to a new compound X. Assuming that all of the nitrogen appears in the new compound, what is the oxidation state of nitrogen in compound X ?

Question

A 2.5 mol of hydrazine N2H4 loses 25 mole of electrons is being converted to a new compound X. Assuming that all of the nitrogen appears in the new compound, what is the oxidation state of nitrogen in compound X ? (A) - 1 (B) - 2 (C) +3 (D) +4

Tardigrade Admin · Accepted Answer

Let the O.N. of N in new compound X be x

N_{2}^{+ 6} H_{4} - - - - - > 2 N^{+ x} + n e^{-}

Let the no. of electrons lost per mole = n

= 2 (- 2) = 2 x + n (- 1)

or n = 2 x + 4 = 2 (x + 2)

=. No. of electron lost per mole = 2(x + 2)
o. of electrons lost by 2.5 moles

= 2.5 \times 2 (2 + x)

Now, 2.5

\times

2 (2 + x) = 25
5 ( 2 + x) = 2 5
or 2 + x = 5 or x = + 3

Q. A 2.5 mol of hydrazine N2​H4​ loses 25 mole of electrons is being converted to a new compound X. Assuming that all of the nitrogen appears in the new compound, what is the oxidation state of nitrogen in compound X ?

- 1

- 2

+3

+4

Q. A 2.5 mol of hydrazine $N_{2} H_{4}$ loses 25 mole of electrons is being converted to a new compound X. Assuming that all of the nitrogen appears in the new compound, what is the oxidation state of nitrogen in compound X ?