What mass of red iron ore containing 80% iron (III) oxide was dissolved in a 200 g nitric acid

| September 15, 2021 | education

What mass of red iron ore containing 80% iron (III) oxide was dissolved in a 200 g nitric acid solution with a mass fraction of HNO3 12.6%?

1. Let’s compose the reaction equation:

Fe2O3 + 6HNO3 = 2Fe (NO3) 3 + 3H2O;

2. Calculate the mass of nitric acid:

m (HNO3) = w (HNO3) * m (solution HNO3) = 0.126 * 200 = 25.2 g;

3. Find the chemical amount of acid:

n (HNO3) = m (HNO3): M (HNO3);

M (HNO3) = 1 + 14 + 3 * 16 = 63 g / mol;

n (HNO3) = 25.2: 63 = 0.4 mol;

4. Determine the amount of reacted iron oxide:

n (Fe2O3) = n (HNO3): 6 = 0.4: 6 = 0.0667 mol;

5. Let’s calculate the mass of the oxide:

m (Fe2O3) = n (Fe2O3) * M (Fe2O3);

M (Fe2O3) = 2 * 56 + 3 * 16 = 160 g / mol;

m (Fe2O3) = 0.0667 * 160 = 10.672 g;

6. Set the mass of red iron ore:

m (cr. l.) = m (Fe2O3): w (Fe2O3) = 10.672: 0.8 = 13.34 g.

Answer: 13.34 g.



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