An excess of gaseous ammonia was passed through a solution of nitric acid with a mass fraction of acid of 42%

An excess of gaseous ammonia was passed through a solution of nitric acid with a mass fraction of acid of 42% and a mass of 600 g. As a result, 300 g of ammonium nitrate was obtained. Calculate the mass fraction of the yield of ammonium nitrate from the theoretically possible.

Given:
ω (HNO3) = 42%
m solution (HNO3) = 600 g
m pract. (NH4NO3) = 300 g
Find: η (NH4NO3) -?
Decision:
1) HNO3 + NH3 => NH4NO3;
2) m (HNO3) = ω (HNO3) * m solution (HNO3) / 100% = 42% * 600/100% = 252 g;
3) n (HNO3) = m (HNO3) / M (HNO3) = 252/63 = 4 mol;
4) n (NH4NO3) = n (HNO3) = 4 mol;
5) m theor. (NH4NO3) = n (NH4NO3) * M (NH4NO3) = 4 * 80 = 320 g;
6) η (NH4NO3) = m practical. (NH4NO3) * 100% / m theor. (NH4NO3) = 300 * 100% / 320 = 93.75%.
Answer: Mass fraction of NH4NO3 yield is 93.75%.