Problem: One of the uses of oxalic acid (H2C2O4) is rust removal. It reacts with rust (Fe2O3) according to the equationFe2O3(aq) + 6 H3C2O4(aq) → 2 H3Fe2(C2O4)3(aq) + 3 H2O(l)Calculate the number of grams of rust (159.7 g/mol) that can be removed by 25.0 mL of a 0.100 M solution of oxalic acid.(A) 0.0665 grams (B) 2.66 grams (C) 0.200 grams(D) 0.400 grams (E) 0.00250 grams

FREE Expert Solution

Use stoichiometry and the balanced equation to determine the mass of rust (Fe2O3) that will react with 25 mL of 0.1 M oxalic acid (H3C2O4)

It can be seen in the balanced equation that 1 mole of Fe2O3 reacts with 6 moles of H3C2O4

Recall that molarity can be calculated as:

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Problem Details

One of the uses of oxalic acid (H2C2O4) is rust removal. It reacts with rust (Fe2O3) according to the equation

Fe2O3(aq) + 6 H3C2O4(aq) → 2 H3Fe2(C2O4)3(aq) + 3 H2O(l)

Calculate the number of grams of rust (159.7 g/mol) that can be removed by 25.0 mL of a 0.100 M solution of oxalic acid.

(A) 0.0665 grams 

(B) 2.66 grams 

(C) 0.200 grams

(D) 0.400 grams 

(E) 0.00250 grams

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