Calculate the mass of nitric acid required to obtain 2.01 kg of calcium nitrate if the product yield is 98%

Calculate the mass of nitric acid required to obtain 2.01 kg of calcium nitrate if the product yield is 98% of the theoretically possible

1. Let’s write down the equality of chemical interaction:

Ca + 2HNO3 = Ca (NO3) 2 + H2.

2. Find the number of moles of calcium nitrate:

2.01 kg = 2010

nprak (Ca (NO3) 2) = m (Ca (NO3) 2) / M (Ca (NO3) 2) = 2010 g / 164 g / mol = 12.26 mol.

ntheor (Ca (NO3) 2) = nprak (Ca (NO3) 2) / η (Ca (NO3) 2) = 12.26 mol / 0.98 = 12.5 mol.

3. Using the equality of chemical interaction, we calculate the number of moles and, as a result, the mass of nitric acid:

n (HNO3) = ntheor (Ca (NO3) 2) * 2 = 12.5 mol * 2 = 25 mol.

m (HNO3) = n (HNO3) * M (HNO3) = 25 mol * 63 g / mol = 1575 g.

Result: m (HNO3) = 1575 g.