1. Calculate the moles of anhydrous (dry) KAI(SO4)2 that were present in the sample. Show all work including units. Question 2 2. Calculate the ratio of moles of H2O to moles of anhydrous KA/(SO4)2. Show all work including units. Note: Report the ratio to the closest whole number. Question3 3. Write the empirical formula for the hydrated KAl(SO4)2, based on your experimental results and answer to Question 2 . Show all work including units. Hint if the ratio of moles of H2O to moles of anhydrous KA2(SO4)2 was 4 , then the empirical formula would be: KAl(SO4)24H2O. 4. Describe any visual differences between the hydrated sample and the dried, anhydrous form. Question 5 5. How would the following errors affect the empirical formula for the compound? That is, will these errors cause the calculated number of moles of water in the hydrate to be artificially high or low? a. The student ran out of time and did not do the second heating. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? b. The student recorded the mass of the cup + sample incorrectly and started with 2.20g of hydrated compound but used 2.00g in the calculations. Explain how this error will affect the calculation for the number of moles of water in the hydrate? Will the final answer be artificially high or low? How do you know? Experiment 1 Data Table 1: Alum Data