Instructions for Side by Side Printing
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- Cut out the notecards by cutting along each horizontal dotted line
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Week 8 - Chemistry
front 1 The predominant intermolecular force between molecules of I₂ is _____ A) ionic bonds. B) dipole-dipole interactions. C) ion-dipole interactions. D) dispersion forces. E) covalent bonds. | back 1 D) dispersion forces. |
front 2 Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance? A) H₂O B) HF C) N(CH₃)₃ D) CH₃CH₂OH E) CH₃NH₂ | back 2 C) N(CH₃)₃ |
front 3 In a molecule of HI, what intermolecular forces are present? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding | back 3 D) dispersion and dipole-dipole |
front 4 Which of the following exhibits dipole-dipole intermolecular forces in a pure substance? A) BF₃ B) CO₂ C) NH₃ D) Br₂ E) CF₄ | back 4 C) NH₃ |
front 5 What intermolecular forces are present between two molecules of CF₃CF₃? A) dispersion only B) dipole-dipole only C) dispersion and dipole-dipole D) dispersion and hydrogen bonding E) dipole-dipole and hydrogen bonding | back 5 A) dispersion only |
front 6  Identify the type or types of intermolecular forces present between molecules of the compound pictured below: A) dispersion only B) dipole-dipole C) hydrogen bonding D) dispersion and dipole-dipole only E) dispersion, dipole-dipole, and hydrogen bonding | back 6 E) dispersion, dipole-dipole, and hydrogen bonding |
front 7 What intermolecular forces are present between two molecules of CH₃CH₂SH? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding | back 7 D) dispersion and dipole-dipole |
front 8 Ammonia and hydrogen fluoride both have unusually high boiling points due to _____ A) dispersion forces. B) dipole-dipole interactions. C) hydrogen bonding. D) ion-dipole interactions. E) low molar masses. | back 8 C) hydrogen bonding. |
front 9 Which of the following would you expect to have the highest boiling point? A) H₂ B) NH₃ C) N₂ D) CH₄ | back 9 B) NH₃ |
front 10 Convert 2.70 atm to torr | back 10  The correct answer is 2050 torr. |
front 11 Convert 532 torr to kPa. Remember that multiple steps may be required in the conversion. | back 11  The correct answer is 70.9 kPa. |
front 12 The pressure in Denver, Colorado averages about 632 mm Hg. How many atmospheres is this? | back 12  The correct answer is 0.832 atm |
front 13 Convert 797 mm Hg to atm | back 13  The correct answer is 1.05 atm. |
front 14 What is Standard Temperature and Pressure (STP)? A) 298.15 K and 1.00 atm B) 273.15 K and 1.00 atm C) 273.15 K and 0.00 atm | back 14 B) 273.15 K and 1.00 atm |
front 15 Convert 750.0 torr to atm. | back 15 0.9868 atm (or 1) |
front 16 Which one of the following is the largest value of pressure? A) 800 torr B) 950 mmHg C) 1.10 atm D) 85.0 kPa | back 16 B) 950 mmHg |
front 17 A fixed container containing an ideal gas is heated. The pressure of the gas increases because A) the gas molecules move faster and strike the walls of the container more often and with more force. B) the gas molecules slow down, striking the walls of the container less often and with less force. C) the gas molecules begin sticking together other and strike the walls of the container with twice the force. D) the gas molecules will melt and fall to the bottom of the container. E) the gas molecules will no longer behave ideally. | back 17 A) the gas molecules move faster and strike the walls of the container more often and with more force. |
front 18 According to the Kinetic Molecular Theory A) The volume of the gas particles will impact the volume available to the gas. B) Gas particles exert pressure by colliding with one another C) The gas particles are moving in circular motions throughout the container. D) The average kinetic energy is proportional to the temperature of the system. | back 18 D) The average kinetic energy is proportional to the temperature of the system. |
front 19 Fundamentally, pressure is defined as force per unit area. What is the source of the force in a gas sample? A) The force is from gravity acting on the particles. B) The force is composed of the sum of the collisions only between gas molecules. C) The force is composed of the sum of the collisions only between the gas molecules and the container. D) The force is composed of the sum of all collisions--between the gas molecules, each other and the container. E) The force was imparted to the container in its initial filling, a transfer of momentum. | back 19 C) The force is composed of the sum of the collisions only between the gas molecules and the container. |
front 20 Which of the following temperatures is the coldest? A) 100 K B) 100 °C C) 100 °F | back 20 A) 100 K |
front 21 A temperature of 103°F or higher is considered a medical emergency. Patient A comes in with a temperature of 38°C. Patient B comes in with a temperature of 313 K. Is either patient having a medical emergency? A) Yes, patient A only. B) Yes, patient B only. C) Yes, both patients. D) No, neither patient. E) Not enough information to determine | back 21 B) Yes, patient B only. |
front 22 How do you convert a Kelvin temperature to Celsius? A) Multiply by 9/5 and then add 32 B) Subtract 273.15 C) Subtract by 32, then multiply by 5/9 D) Add 273.15E) Celsius is always the same as Kelvin | back 22 B) Subtract 273.15 |
front 23 How do you convert a Celsius temperature to Fahrenheit? A) Multiply by 9/5 and then add 32 B) Subtract 273.15 C) Subtract by 32, then multiply by 5/9 D) Add 273.15 E) Celsius is always the same as Fahrenheit | back 23 A) Multiply by 9/5 and then add 32 |
front 24  Read the thermometer given. What would the temperature be in Kelvin? A) 300 K B) 310.2 K C) -236.2 K D) 316.2 K E) 98.6 K | back 24 B) 310.2 K |
front 25 A thermometer reads 18.3 °C. What is the temperature in Fahrenheit? | back 25 64.9 °F |
front 26 A thermometer reads 111.1 K. What is the temperature in °C?-162.05 | back 26 -162.1 °C |
front 27 A thermometer reads 155.5 °F. What is the temperature in °C? | back 27 68.6 °C |
front 28 While traveling in Europe, you see a weather forecast of 20.0°C. What is this temperature in °F? | back 28 68.0 °F |
front 29 A helium balloon initially at room temperature is dunked into a bucket of liquid nitrogen (T = 77 K). Which of the following will occur? A) Volume increases B) Volume decreases C) The number of moles increases D) The number of moles decreases E) Temperature increases | back 29 B) Volume decreases |
front 30 If the pressure on a movable piston of a closed container is doubled, what will happen? A) Temperature will double B) Temperature will double, volume will be cut in half C) Volume will be cut in half D) Temperature and volume will double E) Temperature will increase and volume will decrease, but the specific amount of each cannot be determined with the given information. | back 30 E) Temperature will increase and volume will decrease, but the specific amount of each cannot be determined with the given information. |
front 31 If two separate containers A and B have the same volume and temperature, but container A has more gaseous molecules than B, then container A will have: A) Higher pressure B) Lower pressure C) A greater universal gas constant D) A smaller universal gas constant | back 31 A) Higher pressure |
front 32 What gas law states that volume and pressure are inversely proportional at constant temperature and moles? A) Boyle's Law B) Charles' Law C) Gay-Lussac's Law D) Avogadro's Law E) Combined Gas Law | back 32 A) Boyle's Law |
front 33 A balloon at 30.0°C has a volume of 222 mL. If the temperature is increased to 53.1°C and the pressure remains constant, what will the new volume be, in mL? | back 33 239 mL |
front 34 Which one of the following best describes Charles's Law? A) The volume of a gas is directly proportional to the temperature of the gas. B) The pressure of a gas is directly proportional to the temperature of the gas. C) The volume of a gas is directly proportional to the moles of a gas. D) The pressure of a gas is inversely proportional to the volume of a gas. | back 34 A) The volume of a gas is directly proportional to the temperature of the gas. |
front 35 A 1.20 L weather balloon on the ground has a temperature of 25.0°C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.720 atm, then the new volume is 1.80 L. What is the temperature (in °C) of the air at this elevation? | back 35 49 °C |
front 36 A weather balloon calibrated at 0.00 °C to have a volume of 20.0 L has what volume in L at -40.0 °C assuming pressure is held constant? | back 36 17.1 L |
front 37 One way to measure temperature in some applications is to monitor the gas pressure in a rigid, closed container. What is the temperature (in °C) of such a vessel, calibrated to read 1.00 atm at STP, if the pressure reads 1.25 atm? | back 37 68.29 °C |
front 38 The gas in a 250.0 mL piston experiences a change in pressure from 1.00 atm to 2.80 atm. What is the new volume (in mL) assuming the moles of gas and temperature are held constant? | back 38 89.3 mL |
front 39 15.0 L of an ideal gas at 298 K and 3.36 atm are heated to 383 K with a new pressure of 6.00 atm. What is the new volume in liters? | back 39 10.8 L |
front 40 How many moles of chlorine gas at 120.0 °C and 33.3 atm would occupy a vessel of 12.0 L? | back 40 12.4 mol |
front 41 What is the pressure in atm of a 5.00 L tank with 2.50 moles of oxygen at 39.3 °C? | back 41 12.8 atm |
front 42 What is the temperature (in K) of 0.300 mole of neon in a 2.00 L vessel at 4.68 atm? | back 42 3.80 × 10² K |
front 43 In a 4.00 L pressure cooker, water is brought to a boil. If the final temperature is 115.0 °C at 3.20 atm, how many moles of steam are in the cooker? | back 43 0.402 mol |
front 44 What volume in liters would 20.0 moles of sulfur dioxide occupy at 75.3 °C with a pressure of 3.00 atm? | back 44 191 L |
front 45 A sample of 2.00 mol of gas in a 10.00 L container is at 45.0 °C. What is the pressure (in atm) of the gas? | back 45 5.22 atm |