PS06.MoleIntro

Basic Chemistry (Chapters 1-16)

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CHEMISTRY NAME____________________ PROBLEM SET #6 PERIOD _____________ DIRECTIONS: For each problem that requires a calculation, show the set-up , unit cancellations , and the answer . EXAMPLE: 1.00 x 10 -1 mol X 3.87 x 10 1 g/mol = 3.87 x 10 0 g or 2.00 x 10 2 g 1.00 x 10 2 g/mol = 2.00 x 10 0 mole 1. 3.00 grams of zinc are consumed in an experiment. Calculate how many moles of zinc are consumed. 2. Calculate how many grams of lead (Pb) there are in 5.50 moles of lead. 3. Calulate how many moles of HCl there are in 25.5 grams of HCl. 4. Calulate how many grams of MgCl 2 there are in 10.0 moles of MgCl 2 . 5. A chemist weighs out 10 . 0 grams of chlorine gas (Cl 2 ) and 10 . 0 grams of sulfur dichloride (SCl 2 ). How many moles of each substance does he have? 6. A chemist has 5.00 grams of aluminum. How many moles of aluminum atoms does she have?
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Unformatted text preview: What if she has 0.85 grams of iron? 7. If 16.0 grams of hydrogen gas (H 2 ) were consumed in a reaction, how many moles of H 2 were used? 8. If 144.0 grams of water (H 2 O) were produced in the reaction above (#7)how many moles were produced? 9. Given the information in 7 & 8 above, how many moles of H 2 O are produced for each mole of H 2 consumed? Hint: Set up the appropriate ratio, then make a statement to answer the questions. 10. Using the informationin #9 make a statement for molecules of H 2 O/molecule of H 2 . Explain why we can use moles to answer questions about molecules. 11. Presuming that enough oxygen gas (O 2 ) is available, write a balanced equation for the reaction described in 7 & 8....
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PS06.MoleIntro - What if she has 0.85 grams of iron? 7. If...

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