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# hw7a - Thomas Phillip Homework 7 Due 11:00 pm Inst Brodbelt...

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Thomas, Phillip – Homework 7 – Due: Oct 31 2007, 11:00 pm – Inst: Brodbelt 1 This print-out should have 23 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. The due time is Central time. Brodbelt CH301 Homework 7 Due October 31, 2007 at 11:00 PM 001 (part 1 of 1) 10 points The same number of grams of NH 3 and O 2 are placed in separate bulbs of equal vol- ume and temperature under conditions when both gases behave ideally. Which statement is true? 1. The bulb containing O 2 contains more molecules of gas. 2. The pressure in the O 2 bulb is greater than the pressure in the NH 3 bulb. 3. The pressures in the two bulbs are the same. 4. The pressure in the NH 3 bulb is greater than the pressure in the O 2 bulb. correct 5. Both bulbs contain the same number of moles of gas. Explanation: The molecular weight of NH 3 is less than that of O 2 , so in equal masses there are more moles of NH 3 than of O 2 . At the same volume and temperature, the larger number of moles of NH 3 would exert a higher pressure. 002 (part 1 of 1) 10 points How many molecules are in 1.00 liter of O 2 gas at 56 C and 821 torr. 1. 2 . 24 × 10 23 molec 2. 4 . 00 × 10 - 2 molec 3. 32 molec 4. 1 . 83 × 10 25 molec 5. 2 . 41 × 10 22 molec correct Explanation: V = 1 L T = 56 C + 273 = 329 K P = 821 torr · atm 760 torr = 1 . 08 atm Applying the ideal gas law equation, P V = n R T n = P V R T n = (1 . 08 atm) (1 L) ( 0 . 08206 L · atm mol · K ) (329 K) · 6 . 02 × 10 23 molec 1 mol = 2 . 41 × 10 22 molec 003 (part 1 of 1) 10 points At STP, 6.0 grams of CO gas will occupy a volume of 1. 4.8 liters. correct 2. 5.6 liters. 3. 22.4 liters. 4. 2.24 liters. 5. 3.5 liters. Explanation: T = 0 C + 273 = 273 K P = 1 atm n = 6 g · mol 28 g = 0 . 214 mol Applying the ideal gas law, P V = n R T V = n R T P V = (0 . 214 mol) ( 0 . 08206 L · atm mol · K ) (273 K) 1 atm = 4 . 79411 L 004 (part 1 of 1) 10 points A flask contains 0.123 moles of an ideal gas that occupies 781 mL. A second flask at the same temperature contains 0.0712 moles of

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Thomas, Phillip – Homework 7 – Due: Oct 31 2007, 11:00 pm – Inst: Brodbelt 2 the same gas. The pressure is the same in both flasks. What is the volume of the second flask? 1. 1350 mL 2. 904 mL 3. 452 mL correct 4. 89,180 mL 5. 6.8 mL Explanation: n 1 = 0 . 123 mol n 2 = 0 . 0712 mol V 1 = 781 mL Applying the ideal gas law equation, P V = n R T V 1 V 2 = n 1 n 2 V 2 = V 1 n 2 n 1 V 2 = (781 mL) (0 . 0712 mol) 0 . 123 mol = 452 mL 005 (part 1 of 1) 10 points What is the volume of 0.500 moles of an ideal gas at 273 K and 760 torr? 1. 11.2 liters correct 2. 4.56 cubic fathoms 3. 2.24 liters 4. 380 ml 5. 22.4 liters Explanation: 006 (part 1 of 1) 10 points A 2.00 mole sample of gas is at a temperature of 100.0 C and occupies 3.00 liters. What is its pressure? 1. 20.4 atm correct 2. 0.0500 atm 3. 5.50 atm 4. 0.180 atm 5. The correct answer is not given. Explanation: n = 2 mol T = 100 C + 273 = 373 K V = 3 L Applying the ideal gas law equation, P V = n R T P = n R T V P = (2 mol) ( 0 . 08206 L · atm mol · K ) (373 K) 3 L = 20 . 4 atm 007 (part 1 of 1) 10 points How many moles of HCl gas are produced if 5.00 L of Cl 2 and excess H 2 are reacted at STP?
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