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?

The mass of nitrogen molecule = 45.65 g

Explanation:

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

We know that:

numbers of moles = mass/molar mass

For :

number of moles = 50g/92 g/mol

number of moles = 0.5435 mol

For :

number of moles = 45 g/ 32 g/mol

number of moles = 1.40625 mol

From the above equation;

number of moles of needed = 1/2 moles of  = 1/2 ×  1.40625 mol

= 0.703125 mol

The amount of present = 0.5435 moles which is less than the needed. As such is the limiting reagent

The number of moles of nitrogen molecule produced = 3 × ()

= 3 × 0.5435

= 1.6305  mol

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

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

The mass of nitrogen molecule = 45.654 g

The mass of nitrogen molecule = 45.65 g

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