Question

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?

Answer 1

The mass of nitrogen molecule
`N_2` = 45.65 g

Step-by-step explanation:

The equation for the redox reaction can be represented as follows:

`\mathtt{2N_2H_4 +N_2O_4 \ \to \ 3N_2 + 4H_2O}`

We know that:

numbers of moles = mass/molar mass

For
`\mathtt{N_2O_4}` :

number of moles = 50g/92 g/mol

number of moles = 0.5435 mol

For
`\mathtt{N_2H_4}` :

number of moles = 45 g/ 32 g/mol

number of moles = 1.40625 mol

From the above equation;

number of moles of
`\mathtt{N_2O_4}` needed = 1/2 moles of
`\mathtt{N_2H_4}` = 1/2 × 1.40625 mol

= 0.703125 mol

The amount of
`\mathtt{N_2O_4}` present = 0.5435 moles which is less than the needed. As such
`\mathtt{N_2O_4}` is the limiting reagent

The number of moles of nitrogen molecule
`N_2` produced = 3 × (
`\mathtt{N_2O_4}`)

= 3 × 0.5435

= 1.6305 mol

The mass of nitrogen molecule
`N_2` = number of moles of
`N_2` × molar mass of
`N_2`

The mass of nitrogen molecule
`N_2` = 1.6305 mol × 28 g/mol

The mass of nitrogen molecule
`N_2` = 45.654 g

The mass of nitrogen molecule
`N_2` = 45.65 g