Mass of evaporating dish watch glass and nacl g 6

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5. Mass of Evaporating Dish, Watch Glass, and NaCl (g) 6. Mass of NaCl (g) (Box 5- Box 1) 7. Moles of NaCl (mol) (Based on Box 6) Calculation: Analysis Questions Directions: Show all work, and include all units 1. Calculate the ratio of moles of sodium bicarbonate to moles of sodium chloride that you obtained in your experiment. 2. Based on the reaction written in the Pre-Lab, what is the actual mole ratio of sodium bicarbonate to sodium chloride? 3. a) Using your answer to question 2, how many moles of sodium chloride should you have theoretically obtained? b) How many grams of sodium chloride should you have theoretically obtained? c) How many grams of sodium chloride did you actually obtain? d) We often express yields (amounts of product formed) in terms of a percentage. The percent yield calculation reflection how much of the theoretical amount was actually produced. Calculate the percent yield of sodium chloride. Actual yield (g ) x 100% Theoretical yield (g) 4. How many moles of H 2 O should have theoretically been produced? 5. How many moles of CO 2 should have theoretically been produced? 6. Suppose you started the lab with 5.5 grams of sodium bicarbonate. a) Convert this mass to moles:
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b) Determine the number of moles of sodium chloride you would expect to produce c) How many grams of sodium chloride would you expect to produce? 7. If you wanted to produce exactly 0.75 mol of NaC1, what mass of NaHCO 3 would you start with (assuming a "perfect" procedure)? 8. Suppose you did not evaporate all of the water out of your sodium chloride. How would this affect the results? 9. Why were bubbles produced during the reaction?
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  • Fall '12
  • Pitt
  • Mole, Reaction, sodium bicarbonate, Sodium chloride, Solvay process

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