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Entry Task: Nov. 6 th Tuesday

Entry Task: Nov. 6 th Tuesday. Turn in Lab Get Ch. 10 review signed off. Agenda. Discuss Ch. 10- gases Self-Check- Ch. 1-9 Round robin review CH. 1-10 Exam next time! Bring Book to class.

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Entry Task: Nov. 6 th Tuesday

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  1. Entry Task: Nov. 6th Tuesday Turn in Lab Get Ch. 10 review signed off

  2. Agenda • Discuss Ch. 10- gases • Self-Check- Ch. 1-9 • Round robin review • CH. 1-10 Exam next time! • Bring Book to class

  3. Zinc reacts with HCl to create ZnCl2 and H2. If 34.6g of Zn are reacted with an excess of hydrochloric acid at standard pressure, what is the temperature of the hydrogen gas produced if it occupies a 2.00 dm3 container? Zn + 2HCl  ZnCl2 + H2 P= 1 atm V= 2 L n= convert grams to moles R= 0.08206 T= ? 34.6g/65.39g = 0.529 mol of Zn 0.529 mol of Zn there is a 1 Zn:1 H2 ratio so the same (1)(2) = (0.529)(0.08206)(X) 2 = X 0.0434 = 46K

  4. A balloon is filled with gas at a pressure of 102.3 kPa and a temperature of 45.5°C. Its volume under these conditions is 12.5 L. The balloon is then taken into a decompression chamber where the volume is measured as 2.50 L. If the temperature is 36.0°C, what is the pressure in the chamber? P1=102.3 V1= 12.5 T1=318 P2=X V2= 2.50 T2=309 (102.3)(12.5) 318 (X)(2.50) 309 = = 497kPa

  5. A natural gas tank is constructed so that the pressure remains constant. On a hot day when the temperature was 33.0°C, the volume of gas in the tank was determined to be 3000.0 L. What would the volume be on a cold day when the temperature is 11.0°C? V1= 3000.0 T1=306 V2= X T2=284 3000.0) 306 (X) 284 = = 2780 L

  6. When a sample of a gas was placed in a sealed container with a volume of 3.35 L and heated to 105°C, the gas vaporized and the resulting pressure inside the container was 1.68 atm. How many moles of the gas was present? P=1.68 V= 3.35L n= X R 0.08206 T= 378 5.628 = X 31.019 = 0.181 mol

  7. A 500 mL sample of oxygen was collected over water at 23°C and 760 torr pressure. What volume will the dry oxygen occupy at 23°C and 760 torr? The vapor pressure of water at 23°C is 21.1 torr. Poxygen= PTOTAL – PWATER = 760 torr – 21.1 torr Poxygen= 738.9 torr P1=760 torr V1= 500 ml P2= 738.9 torr V2=X (760)(500) = (738.9 )(x) 514 mL

  8. A 500 mL sample of oxygen was collected over water at 23°C and 760 torr pressure. What volume will the dry oxygen occupy at 23°C and 760 torr? The vapor pressure of water at 23°C is 21.1 torr. P=760 V= 500L n= X R 0.08206 T= 378 5.628 = X 31.019 = 0.181 mol

  9. A molecule of NO2 gas has an average speed of 12.3 m/s at a given temp and pressure. What is the average speed of hydrogen molecules at the same conditions? Set up problem so x is in the numerator on the left hand side of equation 59.0 m/sec

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