how many moles of water are theoretically expected to be present in your weighed sample.

Question

Given that the formula predicts that for every 1 mole of K3[Fe(C2O4)3]•3H2O, 3 moles of H2O are present, calculate how many moles of water are theoretically expected to be present in your weighed sample.

Answer 1

You didn't give us the mass of your weighed sample in this post. If I take it from your previous question, and assume it is 0.104 g and not 104 g, then we have...

Molar mass K3[Fe(C2O4)3]•3H2O = 491.25 g/mol

0.104 g x 1 mol / 491.25 g = 0.0002117 moles = 2.12x10^-4 moles

There are 3 moles of H2O per mole of K3[Fe(C2O4)3]•3H2O, so

moles H2O = 3 x 2.12x10^-4 moles = 6.36x10^-4 moles H2O