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11 Nov 2019
Questions 2-4 I'm lost on how to start. Read the entire procedure, and answer the following questions neatly on a separate piece of paper. 1. Read the section in your textbook regarding hydrates. What is the word used to describe a compound that has had its waters of hydration removed? 2. Calculate the formula weights (in amu) for anhydrous copper(II) sulfate (CuSO_4), copper (II) sulfate trihydrate (CuSO_4 middot 3H_2 O), AND copper(II) sulfate heptahydrate (CuSO_4 middot 7H_2 O). 3. The formula weight is also the molar mass (mass of one mole of the compound), if the units are changed to g/mol. Use your dimensional analysis skills and your value for the molar mass (g/mol) to calculate the number of moles in 3.289 g of copper (II) sulfate trihydrate. 4. Calculate the number of moles in 3.289 g of copper(II) sulfate. Why is this number different from the answer above? 5. When do you stop heating the test tube in Part 1 of the experiment? 6. Why is it necessary to heat a crucible a second time in the quantitative section? 1. What reaction(s) occurs when hydrated salts are heated? 2. How can weight data be used to confirm or deny a hypothesis about a chemical reaction? What happens when hydrated copper (II) sulfate is Write observations and answers to questions on the report sheet and show them to your before continuing on to Part II. Before you start, you should prepare a crucible and lid for part II. Obtain a crucible and
Questions 2-4 I'm lost on how to start.
Read the entire procedure, and answer the following questions neatly on a separate piece of paper. 1. Read the section in your textbook regarding hydrates. What is the word used to describe a compound that has had its waters of hydration removed? 2. Calculate the formula weights (in amu) for anhydrous copper(II) sulfate (CuSO_4), copper (II) sulfate trihydrate (CuSO_4 middot 3H_2 O), AND copper(II) sulfate heptahydrate (CuSO_4 middot 7H_2 O). 3. The formula weight is also the molar mass (mass of one mole of the compound), if the units are changed to g/mol. Use your dimensional analysis skills and your value for the molar mass (g/mol) to calculate the number of moles in 3.289 g of copper (II) sulfate trihydrate. 4. Calculate the number of moles in 3.289 g of copper(II) sulfate. Why is this number different from the answer above? 5. When do you stop heating the test tube in Part 1 of the experiment? 6. Why is it necessary to heat a crucible a second time in the quantitative section? 1. What reaction(s) occurs when hydrated salts are heated? 2. How can weight data be used to confirm or deny a hypothesis about a chemical reaction? What happens when hydrated copper (II) sulfate is Write observations and answers to questions on the report sheet and show them to your before continuing on to Part II. Before you start, you should prepare a crucible and lid for part II. Obtain a crucible and
Casey DurganLv2
25 Mar 2019