theoretical, molar mass, percentage yield Heres my work To figure out the molar mass of CaCl2•H2O (rounding to the hundredths place), I did Ca = 40.08 Cl2 = (35.45) x 2 = 70.9 2H2O = (18.02) x 2 = 36.04 40.08 + 70.90 + 36.04 = 147.02 g/mol 2.97g CaCl•2H2O x (1 mol CaCl•2H2O/147.02g CaCl•2H2O) x (1 mol CaCO3/1 mol CaCl•2H2O) x (100.09/1 mol CaCO3) = 2.04 g (The coefficients were all one, so I used 1 mol in all the neccessary conversion factors.) Now, the third question asked "What is the percent yield of calcium carbonate if your theoretical yield was 2.07 grams" even though I came out with 2.04 g as my theoretical yield. So, percentage yield, (1.46/2.07) X 100 = 70.5%. Was I accurate in all these equations? If not, could you guide me to where I need to make a modification? Thanks!