A student is given a blue copper sulfate hydrate sample. He weighed the sample in a dry-covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. The mass of the empty crucible and lid was found to be 22.652 g earlier. He then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. On cooling, he finds the mass of the crucible, lid, and contents to be 23.403 g. The sample was changed in the process to very light blue anhydrous CuSO4. If there are 100.0 g of hydrate, how many grams of water would be present on it? How many moles of water will there be?
A) 15.0 g, 0.834 mol
B) 17.5 g, 0.972 mol
C) 20.0 g, 1.11 mol
D) 22.5 g, 1.25 mol