Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
`P + 5HNO_3"(conc.) "rarr H_3PO_4 + H_2O + 5NO_2`
If 9.3 g of phosphorus was used in the reaction, calculate :
The volume of nitrogen dioxide produced at S.T.P.
[H = 1, N = 14, P = 31, O = 16]

Explanation

To solve the problem, we need to follow these steps:

### Step 1: Calculate the moles of phosphorus (P)
We are given the mass of phosphorus used in the reaction, which is 9.3 g. The molar mass of phosphorus (P) is given as 31 g/mol.

Using the formula for moles:
\[
\text{Moles of P} = \frac{\text{Given mass}}{\text{Molar mass}} = \frac{9.3 \, \text{g}}{31 \, \text{g/mol}}
...