1. Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. (Type below and show all work to an

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1 Calculate The Moles Of Anhydrous Dry Kal So4 2 That Were Present In The Sample Type Below And Show All Work To An 1 (50.62 KiB) Viewed 14 times

1. Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. (Type below and show all work to answer.) 2. Calculate the ratio of moles of H₂O to moles of anhydrous KAl(SO4)2. Note: Report the ratio to the closest whole number. (Type below and show all work to answer.) 3. Write the empirical formula for the hydrated KAl(SO4)2, based on your experimental results and answer to Question. (Type below and show all work to answer.) 4. Describe any visual differences between the hydrated sample and the dried, anhydrous form. 5. How would the following errors affect the empirical formula for the compound? 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? How do you know? b. The student recorded the mass of the cup + sample incorrectly and started with 2.2 g of hydrated compound but used 2.0 g 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?