From 2 kg of ammonia, 10 kg of a solution of nitrate acid with a mass fraction

| September 8, 2021 | education

From 2 kg of ammonia, 10 kg of a solution of nitrate acid with a mass fraction of 62% were obtained. Calculate the acid yield as a percentage of the theoretically possible.

Given: m (NH3) = 2 kg = 2000 g m solution practical. (HNO3) = 10 kg = 10000 g ω (HNO3) = 62% Find: ω out. (HNO3) -?
Solution:
1) Write the reaction equation: NH3 + 2O2 => HNO3 + H2O; 2) Find the amount of substance NH3: n (NH3) = m (NH3) / Mr (NH3) = 2000/17 = 117.6 mol; 3) Find the amount of substance HNO3: n (HNO3) = n (NH3) = 117.6 mol; 4) Find the theoretical mass of HNO3: m theor. (HNO3) = n (HNO3) * Mr (HNO3) = 117.6 * 63 = 7408.8 g; 5) Find the practical mass of HNO3: m practical. (HNO3) = ω (HNO3) * m solution practical. (HNO3) / 100% = 62% * 10000/100% = 6200 g; 6) Find the output of HNO3: ω out. (HNO3) = m practical (HNO3) * 100% / m theor. (HNO3) = 6200 * 100% / 7408.8 = 84%.
Answer: The HNO3 yield was 84%.



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