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Stoichiometric Calculations

What mass in ...

Question

What mass (in gram) (as nearest integer) of $N_{2} H_{4}$ can be oxidised to $N_{2}$ by $24.0$ g of $K_{2} C r O_{4}$ which is reduced to $[C r (O H)_{4}]^{-}$ ?

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Solution

The oxidation number of chromium changes from $+ 6$ to $+ 3$ .
The oxidation number of each $N$ atom changes from $- 2$ to $0$ .
Net increase in the oxidation number of two $N$ atoms in hydrazine $= 4$ .
Thus, $3$ moles of hydrazine $= 4$ moles of $K_{2} C r O_{4}$ .
Molar mass of hydrazine is $32$ g/mol.
Molar mass of potassium chromate is $194.19$ g/mol.
The mass of hydrazine that can be oxidized is $\frac{3}{4} \times \frac{24.0 g}{194.19 g / m o l} \times 32 g / m o l = 2.969 g = 3 g$ .

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