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from bathtub rings via the following quantitatively correct equation: .

4 H (aq) + Fe2 03(S)+ C2 H2 04(aq) 2 Fe(aq)+ C2 04(aq) + 3 H2 0 (1)

Calculate the mass in grams of rust that may be removed from a ring ridden bathtub via the application of 500 mL of a

0.370 M solution of oxalic acid.

For this problem I 500x10^3 L C2H204 x .37 mol C2H2O4/i L c2h2o4 = .185 mol C2H2O4

then I .185 C2H2O4 x 2 mol Fe/ a mol C2H2O4 x 55.84 g Fe / mol Fe = 20.7 grams of Fe

this seems right to me but at the same time I'm still kind of 'rusty' with chemistry and I wanted to see if any one knew if this was correct and if it is wrong oculd lead me in the right direction?