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Balancing Chemical Equations by Hit and Trial Method

HNO3 oxidises...

Question

$H N O_{3}$ oxidises $N H_{4}^{+}$ ions to nitrogen and itself gets reduced to $N O_{2}$ . The moles of $H N O_{3}$ required by $1 m o l$ of $(N H_{4})_{2} S O_{4}$ is?

4

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5

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6

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2

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Solution

The correct option is A $4$
Given :
solution :the balanced chemical equation be :

$(N H_{4})_{2} S O_{4} + 6 H N O_{3} \to N_{2} + 6 N O_{2}$
from this equation we can clearly say that one mole of $(N H_{4})_{2} S O_{4}$ utilises 6 moles of $N O_{2}$
hence the correct opt: C

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