Question

Data Table 1. CuSO4 Data Mass of empty cup (grams) Mass of CuSO, hydrate (erams)S Cuso, hydrate after 1st heating (grams) CuSO, hydrate after 2nd heating (grams) Mass of released H20 (grams) Number of moles of released H201 Mass of anhydrous Cuso (grams) Number of moles of anhydrous CuSO 02a mo Questions: A) Calculate the ratio of moles of H2O to moles of anhydrous Cuso4. Note: Report the ratio to the closest whole number. B) Write the empirical formula for the Cusos hydrate based on your experimental results and answer to Question A. Hint: if the ratio of moles of H0 to moles of anhydrous CuSO4 was x then the empirical formula would be: CuSO4 xH20. C) Describe any visual differences between the hydrated CuSOs and the anhydrous form. D) How would the following errors affect the empirical formula for the compound if a. The student ran out of time and did not do the second heating. b. The student did not subtract the mass of the cup in the calculations. A chemist is given a sample of the CusO, hydrate and was asked to determine its empirical formula. The original sample weighed 42.75 g. After heating to remove the water of hydration, the sample weighed 27.38 g. Determine the formula for this hydrate. E)

Answer 1

1 T.hea HalM Ye lea reol H20-1.0ay. ー No 4-rnoles arh olYos G. çoys 3.qqr 1:2.3 CAL 29 hy dro s Ca Soy fnkas hich vhite and in th (CAO, İç 늬ue Ib Colouý.dk

dvou^) . -final farmi a Cafoy ehow( lenen no9-moluą.cod.. ltanea. Ђ hydrated Ca Soy maq 41.75 g 4 29.36g Atter Ho hemoyed о.ms. 4.1a