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Question

Hydrazine (N2H4) is a rocket fuel which can be produced according to the following reaction:


ClNH2+2NH3N2H4+NH4Cl

When 1000 g of ClNH2 is reacted with excess of NH3, 473 g of N2H4 is produced. What is the percentage yield of the reaction?

A
76.12
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B
67.21
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C
26.17
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D
16.72
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Solution

The correct option is A 76.12
1 mole of ClNH2 reacts to form 1 mole of N2H4.

The molar mass of ClNH2 is 35.5+14+2=51.5 g/mol
The molar mass of N2H4 is 2(14)+4=32 g/mol

Thus, 51.5 g of ClNH2 reacts to form 32 g of N2H4.

Thus, 1000 g of ClNH2 reacts to form 32×100051.5=621.36 g of N2H4.

However, only 473 g of N2H4 are obtained.

Hence, the percentage yield of the reaction is 473621.36×100=76.12%.

Therefore, option A is correct.

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