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

Answer:

The mass of nitrogen molecule $N_2$ = 45.65 g

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