dinitrogen tetroxide and hydrazine (n2h4) undergo a redox reaction in which nitrogen and water are formed as products. what mass of nitrogen could be produced when 50.0 g of dinitrogen tetroxide and 45.0 g of hydrazine are combined? report your answer to the appropriate number of significant figures.

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15-12-2022
Chemistry

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dinitrogen tetroxide and hydrazine (n2h4) undergo a redox reaction in which nitrogen and water are formed as products. what mass of nitrogen could be produced when 50.0 g of dinitrogen tetroxide and 45.0 g of hydrazine are combined? report your answer to the appropriate number of significant figures.

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abhinavjh321 abhinavjh321 · Answer 1 · 2022-12-21T02:47:29-05:00

Nitrogen and water are produced as byproducts of a redox process involving dinitrogen tetroxide and hydrazine (N2H4). 45.7g of nitrogen might potentially be created.

The following is a representation of the redox reaction's equation:

N2O4 + 2N2H4 = 3N2 + 4H2O

We are aware of: The formula for moles is mass/molar mass.

Given mass of dinitrogen tetroxide = 50g

mass of hydrazine = 45g

Number of moles for N2O4 = 50/92,where N2O4 has a molar mass of 92

number of moles = 0.5435 mol.

Number of moles for N2H4 = 45/32, where N2H4 has a molar mass of 32

number of moles = 1.40.

Given the previous equation:

Half of a mole of N2H4 is equal to 1.40625 moles of N2O4, = 0.703125 moles.

0.5435 moles of N2O4 are present, which is less than what is required.

N2O4 is the limiting reagent as a result.

The number of moles of nitrogen molecule N2 produced = 3XN2O4 = 3X0.5435 = 1.6305

The mass of nitrogen molecule = number of moles of N2 × molar mass of N2 = 1.6305 mol × 28 g/mol = 45.7g

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