Answer: 145.87 grams of ammonia will produce the given amount of nitrogen.
Explanation:
To calculate the moles of nitrogen, we use the formula:
\(\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}\) ....(1)
Given mass of nitrogen = 300 g
Molar mass of nitrogen = 28.02 g/mol
Putting values in above equation, we get:
\(\text{Moles of nitrogen}=\frac{300g}{28.02g/mol}=10.706mol\)
For the given reaction:
\(4NH_3+6NO\rightarrow 5N_2+6H_2O\)
By Stoichiometry of the reaction:
5 moles of nitrogen is produced from 4 moles of ammonia.
So, 10.706 moles of nitrogen will be produced from = \(\frac{4}{5}\times 10.706mol=8.564mol\)
Now, calculating the mass of ammonia, we use equation 1:
Molar mass of ammonia = 17.0337 g/mol
Moles of ammonia = 8.564 mol
Putting values in equation 1, we get:
\(8.564mol=\frac{\text{Mass of ammonia}}{17.0337g/mol}\\\\\text{Mass of ammonia}=145.87grams\)
Hence, 145.87 grams of ammonia will produce the given amount of nitrogen
