Practice Exam 2 (2)

# Practice Exam 2 (2) - 8. Precip Reactions: Give the...

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Practice Exam 2 – Chapters 3b, 4, and 5 Chapter 3 1. mass to mass: 2 CuO + C -> 2 Cu + CO 2 What mass in g of copper is produced when 100.0 g of carbon is used? 2. limiting reagent: 2 CuO + C -> 2 Cu + CO 2 If the reaction is run with 40.0 g of copper (II) oxide and 20.0 g of carbon, what is the limiting reagent? 3. percent yield: 2 CuO + C -> 2 Cu + CO 2 If the reaction is run with 25.0 g of carbon, and the product yield is only 12.0 g of copper, what is the percent yield for the reaction? Chapter 4 4. Molarity: You need to make a solution of 3.0 L of 5.0 M NaOH from solid NaOH. How many grams of NaOH should you use? 5. Molarity: You need to make a solution by diluting a stock solution of 6.0 M NaOH. You need 3.0 L of 5.0 M NaOH. How much of the 6.0 M solution do you dilute? 6. Acid/Bases: Give the products and balance: Mg(OH) 2 + HCl -> 7. If you were doing a titration in the lab, and you used 25.0 mL of 0.2M NaOH to neutralize 40.0 mL of an acid of unknown concentration, what was the concentration of your acid?
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Unformatted text preview: 8. Precip Reactions: Give the products, phases, and balance: CaCl 2 + Na 2 SO 4-> 9. Redox: Balance Sn + NO 3--> SnCl 6 2-+ NO 2 Chapter 19 10. Nuclear Reactions: Balance 14 N + 4 He -> ___ + 1 H Chapter 5 11. Situation: You have a tank. It has 4.0 moles of gas at 300.0 K and 3.5 atm of pressure. What is the volume? 12. Initial/Final: You have a tank. The temperature is 425 K and has a pressure of 5.6 atm. You heat the tank to 515 K. What is the new pressure? 13. Dalton: You have a tank. It has three gases, 3.0 moles of helium, 2.0 moles of hydrogen, and 4.0 moles of fluorine. The tank is 50.0 L and the temperature is 213 K. What is the total pressure and the partial pressure of all of the gases? 14. Density: What is the density of neon at 355 K and 1.0 atm? 15. Density: What is the molecular weight of a gas that has a 1.34 g/L at STP?...
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## This note was uploaded on 03/24/2012 for the course CHM 131 taught by Professor Goodmen during the Fall '12 term at Moraine Valley Community College.

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