THIS IS Chapter 13 Jeopardy

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Jeopardy Gas Stoichiometry Matching/ Vocab Boyles Law Charles Law Ideal Gas Law Other Gas Laws 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500

A gas occupies a volume of 202 mL at a pressure of 505 torr A gas occupies a volume of 202 mL at a pressure of 505 torr. To what pressure must the gas be subjected in order to change the volume to 65.0 mL? Assume constant temperature. A 100

1570 torr; 2.07 atm A 100

A sample of helium gas occupies 2. 65 L at 1. 20 atm A sample of helium gas occupies 2.65 L at 1.20 atm. What pressure would this sample of gas exert in a 1.50-L container at the same temperature? A 200

2.12 atm A 200

Define Boyle’s Law A 300

At constant temperature, the volume of a given amount of gas is inversely proportinal to its pressure A 300

A gas has a volume of 5. 0 L at a certain pressure A gas has a volume of 5.0 L at a certain pressure. How must the pressure be changed to double the volume of the gas at constant temperature? A 400

The pressure must be halved

The pressure of a sample of gas is 500. mm Hg and the volume is 30.0 L. If the volume is changed to 50.0 L, what is the new pressure? A 500

833 mm Hg A 500

A balloon has a volume of 1. 20 L at 24. 0°C A balloon has a volume of 1.20 L at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon. B 100

1.30 L B 100

A gas sample is held at constant pressure. The gas occupies 3 A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.45 L. B 200

281 K B 200

Define Charles’s Law B 300

At constant pressure, the volume of a given amount of gas is directly proportional to its kelvin temperature B 300

A balloon has a volume of 1. 20 L at 24. 0°C A balloon has a volume of 1.20 L at 24.0°C. The balloon is heated to 48.0°C. Calculate the new volume of the balloon. B 400

1.30 L B 400

A sample of gas has a volume of 50. 0 L at a temperature of 300. K A sample of gas has a volume of 50.0 L at a temperature of 300. K. What temperature would be needed for this sample to have a volume of 60.0 L if its pressure remains constant? B 500

87 °C B 500

A sample of an ideal gas containing 0 A sample of an ideal gas containing 0.954 mol is collected at 742 torr pressure and 31°C. Calculate the volume. C 100

24.4 L C 100

A 36.0-g sample of acetylene, C2H2(g), at STP is subject to a new temperature and pressure of 35°C and 805 mm Hg. Calculate the volume of the acetylene under these new conditions. C 200

33.0 L C 200

What volume will 28.0 g of N2 occupy at STP?

22.4 L C 300

DAILY DOUBLE DAILY DOUBLE Place A Wager C 400

What volume is occupied by 19. 6 g of methane, CH4, at 27°C and 1 What volume is occupied by 19.6 g of methane, CH4, at 27°C and 1.59 atm? C 400

18.9 L C 400

A 4.40-g piece of solid CO2 (dry ice) is allowed to vaporize (change to CO2(g)) in a balloon. The final volume of the balloon is 1.00 L at 300. K. What is the pressure of the gas? C 500

2.46 atm C 500

C2H4 reacts with O2 according to the following equation: C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) What volume of oxygen at STP is needed to react with 1.50 mol of C2H4? D 100

101 L D 100

How many liters of HCl(g) measured at STP can be produced from 4 How many liters of HCl(g) measured at STP can be produced from 4.00 g of Cl2 and excess H2 according to the following equation: H2(g) + Cl2(g) → 2HCl(g) D 200

2.53 L D 200

How many moles of O2(g) are needed to react completely with 52 How many moles of O2(g) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO2(g) and H2O(g) according to the following reaction: CH4(g) + 2O2 → CO2(g) + 2H2O(g) D 300

4.64 moles D 300

What volume of carbon dioxide will be produced from the combustion of 4.50 moles of propane (C3H8) at STP? D 400

302 L D 400

Calcium carbonate decomposes when heated to form calcium oxide and carbon dioxide. What volume of carbon dioxide can be produced from 37.0 g of calcium carbonate at a temperature of 25 °C and a pressure of 1.15 atm? D 500

7.87 L CO2 D 500

A helium balloon has a volume of 2.30 L at 23.5°C and a pressure of 1.00 atm at sea level. The balloon is released and floats upward. At a certain height the atmospheric pressure is 0.810 atm and the temperature is 12.0°C. Calculate the volume of the balloon. E 100

2.73 L E 100

independent of each other b. directly proportional If temperature and pressure are held constant, the volume and number of moles of a gas are independent of each other b. directly proportional c. inversely proportional d. equal E 200

b. directly proportional

A gas originally occupying 10. 1 L at 0 A gas originally occupying 10.1 L at 0.925 atm and 25°C is changed to 12.2 L at 625 torr. What is the new temperature in °C? E 300

47 °C E 300

A mole of a gas at STP has a volume of 22. 4 L A mole of a gas at STP has a volume of 22.4 L. If the volume increases to 29.1 L and the pressure is changed to 813 torr, calculate the new temperature. E 400

379 K E 400

3. 50 g of CO2 and 11. 6 g of O2 are placed in a 3 3.50 g of CO2 and 11.6 g of O2 are placed in a 3.00 L container at 273 K. What will the total pressure in the container be? E 500

3.30 atm E 500

absolute zero F 100

Temperature at which a gas theoretically occupies zero volume F 100

Universal gas constant F 200

0.08206 L·atm/(mol·K) F 200

Define Avogadro’s Law F 300

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas F 300

Define Dalton’s law of partial pressure

The total pressure of a mixture of gases is the sum of the pressures that each gas would exert if alone in the container F 400

What is the molar volume of ideal gas at STP

22.4 liters F 500

The Final Jeopardy Category is: Dalton’s Law of Partial Pressures Click on screen to begin

Click on screen to continue Consider the following: you have 2 liters of neon gas at a pressure of 2 atmospheres, 2 liters of carbon dioxide gas at a pressure of 3 atmospheres, and 2 liters of nitrogen gas at a pressure of 4 atmospheres. All three samples are at room temperature. If you transfer all 3 gases to the same rigid 2 liter container, what is the pressure exerted by the nitrogen in the final mixture? What is the total pressure exerted by the gas mixture? Click on screen to continue

Click on screen to continue 4 atm 9 atm Click on screen to continue

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