Gas Laws REVIEW GAME

Question 1 A 4.3 liter tank of hydrogen is at a pressure of 6.2 atmospheres. What volume of hydrogen will be available if the hydrogen is used at pressure of 0.48 atmospheres? A 4.3 liter tank of hydrogen is at a pressure of 6.2 atmospheres. What volume of hydrogen will be available if the hydrogen is used at pressure of 0.48 atmospheres? Boyle’s Law Boyle’s Law (4.3)(6.2) = 0.48V 2 (4.3)(6.2) = 0.48V 2 V 2 = 56 L V 2 = 56 L

Question 2 What mass of oxygen gas must be placed in a container with a volume of 123.0L to produce a pressure of 1.87 atmospheres at 28.0°C? What mass of oxygen gas must be placed in a container with a volume of 123.0L to produce a pressure of 1.87 atmospheres at 28.0°C? Ideal Gas Law Ideal Gas Law 1.87(123) = n(0.0821)(301) 1.87(123) = n(0.0821)(301) n = 9.3 mol x 32 = 298 g n = 9.3 mol x 32 = 298 g

Question 3 What is the pressure of 20.9 grams of neon gas at -19°C in a rigid container whose volume is 19.0 L? What is the pressure of 20.9 grams of neon gas at -19°C in a rigid container whose volume is 19.0 L? Ideal Gas Law Ideal Gas Law 20.9 g Ne / 20 = mol 20.9 g Ne / 20 = mol P(19) = 1.045(0.0821)(254) P(19) = 1.045(0.0821)(254) P = 1.2 atm P = 1.2 atm

Question 4 A 4.45 L balloon at 14°C contains carbon dioxide gas. If the balloon is taken outside where the temperature is -22°C, what volume will the balloon occupy? A 4.45 L balloon at 14°C contains carbon dioxide gas. If the balloon is taken outside where the temperature is -22°C, what volume will the balloon occupy? Charles Law Charles Law 4.45 / 287 = V 2 / / 287 = V 2 / 251 V 2 = 3.9 L V 2 = 3.9 L

Question 5 A gas occupies a volume of 0.65 L at kPa and a temperature of 0.00°C. What volume will the gas occupy at 2.50 atm and 50.0°C? A gas occupies a volume of 0.65 L at kPa and a temperature of 0.00°C. What volume will the gas occupy at 2.50 atm and 50.0°C? Combined Gas Law Combined Gas Law kPa x (1 atm/ kPa) = 1.17 atm kPa x (1 atm/ kPa) = 1.17 atm 1.17(0.65)/273 = 2.5V 2 / (0.65)/273 = 2.5V 2 /323 V 2 = 0.36 L V 2 = 0.36 L

Question 6 A sample of gas occupies 25 mL at -142°C. What volume does the sample occupy at 65°C? A sample of gas occupies 25 mL at -142°C. What volume does the sample occupy at 65°C? Charles Charles 25/131 = V 2 /338 25/131 = V 2 /338 V 2 = 65 mL V 2 = 65 mL

Question 7 When a container is filled with grams of H 2, grams of O 2, and grams of N 2, the pressure in the container is 5412 kPa. What is the partial pressure of O 2 ? When a container is filled with grams of H 2, grams of O 2, and grams of N 2, the pressure in the container is 5412 kPa. What is the partial pressure of O 2 ? Dalton’s Law Dalton’s Law 6 g H 2 /2 = 3mol 64g O 2 /32 = 2mol 28 g N 2 /28 = 1mol 6 g H 2 /2 = 3mol 64g O 2 /32 = 2mol 28 g N 2 /28 = 1mol = 6 total moles = 6 total moles P O2 = 2/6(5412) = 1804 kPa P O2 = 2/6(5412) = 1804 kPa

Question 7.5 Magnesium reacts with hydrochloric acid Magnesium reacts with hydrochloric acid Mg + 2HCl  MgCl 2 + H 2 Mg + 2HCl  MgCl 2 + H 2 How many grams of magnesium would I have to start with to make 3.5L of hydrogen gas at 130 kPa and 50. degrees celsius? How many grams of magnesium would I have to start with to make 3.5L of hydrogen gas at 130 kPa and 50. degrees celsius? 130(3.5) = n (8.314)(323) 130(3.5) = n (8.314)(323) n = 0.17 mol H 2 x 1/1 x 24.3 = 4.1 g n = 0.17 mol H 2 x 1/1 x 24.3 = 4.1 g

Question 8 What is the volume occupied by 71.0 grams of chlorine gas at STP? What is the volume occupied by 71.0 grams of chlorine gas at STP? Ideal Gas Law Ideal Gas Law 71 g Cl 2 / 71 = 1 mol 71 g Cl 2 / 71 = 1 mol 1V = 1(0.0821)(273) 1V = 1(0.0821)(273) V = 22.4 L V = 22.4 L

Question 9 A rigid container of O 2 has a pressure of 185 kPa at a temperature of 458 K. What is the pressure at 283 K? A rigid container of O 2 has a pressure of 185 kPa at a temperature of 458 K. What is the pressure at 283 K? Gay Lussac’s Law Gay Lussac’s Law 185/458 = P 2 / /458 = P 2 / 283 P 2 = 114 kPa P 2 = 114 kPa

Question 10 An unknown gas moves three times as fast as sulfur dioxide gas. What is the mass of the unknown gas? An unknown gas moves three times as fast as sulfur dioxide gas. What is the mass of the unknown gas? S u = 3 m u = ? S u = 3 m u = ? S so2 = 1 m so2 = 64 S so2 = 1 m so2 = 64 1/3 = Sqrt(m/64) 1/3 = Sqrt(m/64) m = 7.1 g/mol m = 7.1 g/mol

Question 11 How many moles of N 2 are in a flask with a volume of 125 mL at a pressure of 2550 mm Hg and a temperature of K? How many moles of N 2 are in a flask with a volume of 125 mL at a pressure of 2550 mm Hg and a temperature of K? Ideal Gas Law Ideal Gas Law 2550 mm Hg ( 1 atm / 760 mm Hg) = 3.36atm 2550 mm Hg ( 1 atm / 760 mm Hg) = 3.36atm 3.36 (0.125) = n (0.0821) ( 300) 3.36 (0.125) = n (0.0821) ( 300) mol N mol N 2

Question 12 The volume of a gas is 125 mL at 254 kPa pressure. What will the volume be when the pressure is reduced to 1.78 psi, assuming the temperature remains constant? The volume of a gas is 125 mL at 254 kPa pressure. What will the volume be when the pressure is reduced to 1.78 psi, assuming the temperature remains constant? Boyle’s Law Boyle’s Law 254 kPa ( 14.7psi / kPa) = psi 254 kPa ( 14.7psi / kPa) = psi 36.85(125) = 1.78V 36.85(125) = 1.78V V = 2590 mL V = 2590 mL

Question 13 A mixture of gases at a total pressure of 95 kPa contains N 2, CO 2, and O 2. The partial pressure of CO 2 is 24 kPa and the partial pressure of the N 2 is 48 kPa. What is the partial pressure of the O 2 ? A mixture of gases at a total pressure of 95 kPa contains N 2, CO 2, and O 2. The partial pressure of CO 2 is 24 kPa and the partial pressure of the N 2 is 48 kPa. What is the partial pressure of the O 2 ? Dalton’s Law Dalton’s Law 95 = P o2 95 = P o2 P o2 = 23 kPa P o2 = 23 kPa

Question 14 A gas, collected over water, has a measured pressure of 1.23 atm and has a volume of 590 mL at a temperature of 47°C. What volume will the dry gas occupy at 25°C and standard pressure? A gas, collected over water, has a measured pressure of 1.23 atm and has a volume of 590 mL at a temperature of 47°C. What volume will the dry gas occupy at 25°C and standard pressure? Dalton and Combined Dalton and Combined 1.23 atm ( kPa / 1atm ) = kPa 1.23 atm ( kPa / 1atm ) = kPa kPa = P gas kPa = P gas P gas = kPa P gas = kPa (590) / 320 = (V 2 ) / (590) / 320 = (V 2 ) / mL 620 mL

Question 15 Nitrogen gas diffuses into an empty container at a rate of 254 m/s. At what velocity will carbon monoxide gas move at the same temperature? Nitrogen gas diffuses into an empty container at a rate of 254 m/s. At what velocity will carbon monoxide gas move at the same temperature? Graham Graham V CO / 254 = Sqrt (28/28) V CO / 254 = Sqrt (28/28) V CO = 254 m/s V CO = 254 m/s

Question 16 A gas initially is present, in a balloon, at 25°C under 1 atmosphere of pressure. The volume of the gas under these conditions is 2.5L. What will be the new volume of the gas if it is taken outside on a hot day, where the temperature is 85°C and the pressure is 1.08 atmospheres? A gas initially is present, in a balloon, at 25°C under 1 atmosphere of pressure. The volume of the gas under these conditions is 2.5L. What will be the new volume of the gas if it is taken outside on a hot day, where the temperature is 85°C and the pressure is 1.08 atmospheres? Combined Combined 1(2.5)/298 = 1.08V 2 /358 1(2.5)/298 = 1.08V 2 /358 V 2 = 2.8 L V 2 = 2.8 L

Question mL of O 2 gas is collected over water at atm and 10.0°C. What would be the volume of this dry gas at standard conditions? 93.0 mL of O 2 gas is collected over water at atm and 10.0°C. What would be the volume of this dry gas at standard conditions? Dalton and Combined Dalton and Combined atm x ( kPa / 1atm) = kPa atm x ( kPa / 1atm) = kPa kPa = P gas kPa = P gas P gas = 93 kPa P gas = 93 kPa 93(93)/283 = V 2 /273 93(93)/283 = V 2 /273 V 2 = 82.3 mL V 2 = 82.3 mL

Question 18 If 9.0 moles of nitrogen gas will fill a balloon that is 2.0 L in volume at 293 K, what volume will 28 moles of nitrogen gas fill at the same temperature? If 9.0 moles of nitrogen gas will fill a balloon that is 2.0 L in volume at 293 K, what volume will 28 moles of nitrogen gas fill at the same temperature? Avogadro’s Law Avogadro’s Law 2/9 = V 2 / 28 2/9 = V 2 / L 6.2 L

Question 19 A large cylinder of He gas, such as that used to inflate balloons, has a volume of 25.0 L at 22°C and 5.6 atm. How many grams of He are in such a cylinder? A large cylinder of He gas, such as that used to inflate balloons, has a volume of 25.0 L at 22°C and 5.6 atm. How many grams of He are in such a cylinder? Ideal Ideal 5.6(25) = n(0.0821)(295) 5.6(25) = n(0.0821)(295) 5.78 mol x 4 = 23 g 5.78 mol x 4 = 23 g

Question 20 I begin with 460 mL of oxygen gas at a pressure of 740 mm Hg. How many liters of gas are present at standard pressure? I begin with 460 mL of oxygen gas at a pressure of 740 mm Hg. How many liters of gas are present at standard pressure? Boyle Boyle 740(460) = 760(V 2 ) 740(460) = 760(V 2 ) V 2 = 450 mL V 2 = 450 mL

Question 21 Calculate the pressure of a gas whose temperature is increased from 15°C to 25°C and whose original pressure is 0.75 atm. Calculate the pressure of a gas whose temperature is increased from 15°C to 25°C and whose original pressure is 0.75 atm. Gay Lussac Gay Lussac.75/288 = P 2 /298.75/288 = P 2 /298 P 2 = 0.78 atm P 2 = 0.78 atm

Question 22 A sample of gas at standard temperature and pressure is put into an expandable container. The original volume of the gas is 250 mL. What is the new volume if the gas is cooled to -15°C and the pressure is increased to 780 mm Hg? A sample of gas at standard temperature and pressure is put into an expandable container. The original volume of the gas is 250 mL. What is the new volume if the gas is cooled to -15°C and the pressure is increased to 780 mm Hg? Combined Combined (760)(250)/273 = 780V 2 /258 (760)(250)/273 = 780V 2 /258 V 2 = 230 mL V 2 = 230 mL

Question 23 A balloon is filled with 150. mL of carbon dioxide gas at 900. mm Hg and 25.0°C. If the pressure is held constant, what will the new volume be if the temperature is raised to 75.0°C? A balloon is filled with 150. mL of carbon dioxide gas at 900. mm Hg and 25.0°C. If the pressure is held constant, what will the new volume be if the temperature is raised to 75.0°C? Charles Charles 150/298 = V 2 / /298 = V 2 /348 V 2 = 175 mL V 2 = 175 mL

Question 24 Sulfur dioxide gas can move with a velocity of 150 m/s. How fast will carbon dioxide gas move at the same temperature? Sulfur dioxide gas can move with a velocity of 150 m/s. How fast will carbon dioxide gas move at the same temperature? Graham Graham V 1 /150 = Sqrt(64/44) V 1 /150 = Sqrt(64/44) 180 m/s 180 m/s

Question 25 6 moles of nitrogen gas is placed in a 3 L container. What volume will 18 moles of gas occupy under the same conditions 6 moles of nitrogen gas is placed in a 3 L container. What volume will 18 moles of gas occupy under the same conditions Avogadro Avogadro 3/6 = V 2 /18 3/6 = V 2 /18 9 L 9 L

Question g of neon gas is put into a 500. mL container at 15.0°C. What is the pressure within the container in kPa? 40.0g of neon gas is put into a 500. mL container at 15.0°C. What is the pressure within the container in kPa? Ideal Ideal 40 g Ne / 20 = 2 mol 40 g Ne / 20 = 2 mol P(.5) = 2(8.314)(288) P(.5) = 2(8.314)(288) 9580 kPa 9580 kPa

Question 27 If a gas begins at a temperature of 27°C and a pressure of 150 kPa, what will the new pressure be when the temperature is raised to 50.°C? If a gas begins at a temperature of 27°C and a pressure of 150 kPa, what will the new pressure be when the temperature is raised to 50.°C? Gay Lussac Gay Lussac 150/300 = P 2 / /300 = P 2 / kPa 160 kPa

Question 28 Hydrogen gas moves with a velocity of 400. m/s at 25°C. What is the mass of a gas that moves at 250. m/s at the same temperature? Hydrogen gas moves with a velocity of 400. m/s at 25°C. What is the mass of a gas that moves at 250. m/s at the same temperature? Graham Graham 400/250 = Sqrt(m 2 /2) 400/250 = Sqrt(m 2 /2) 5.12 g/mol 5.12 g/mol

Question 29 Oxygen gas is collected over water at 18°C at a pressure of 800. mm Hg and a volume of 100. mL. What is the volume of the dry gas at STP? Oxygen gas is collected over water at 18°C at a pressure of 800. mm Hg and a volume of 100. mL. What is the volume of the dry gas at STP? Dalton and Combined Dalton and Combined 800 mmHg x ( kPa/760 mmHg) = kPa 800 mmHg x ( kPa/760 mmHg) = kPa = P gas = P gas kPa kPa 104.6(100)/291 = V 2 / (100)/291 = V 2 /273 V 2 = 97 mL V 2 = 97 mL

Question 29 6Li + N 2  2Li 3 N 6Li + N 2  2Li 3 N I have 40.0 grams of lithium metal. How many liters of nitrogen gas will react with it at 230. kPa and 17.0 degrees celsius? I have 40.0 grams of lithium metal. How many liters of nitrogen gas will react with it at 230. kPa and 17.0 degrees celsius? 40g/7 x 1/6 = 0.95 mol 40g/7 x 1/6 = 0.95 mol 230(v) = 0.95(8.314)(290) 230(v) = 0.95(8.314)(290) V = 9.95 L V = 9.95 L I have 25.0 L of nitrogen gas at 1.34 atm and 80.0 degrees celsius. How many grams of Li 3 N can I make? I have 25.0 L of nitrogen gas at 1.34 atm and 80.0 degrees celsius. How many grams of Li 3 N can I make? 1.34(25) = n (0.0821)(353) 1.34(25) = n (0.0821)(353) n = 1.15 mol N 2 x 2/1 x 35 = 80.5 g n = 1.15 mol N 2 x 2/1 x 35 = 80.5 g

Question 30 I have 80. grams of carbon monoxide gas, 55 grams of dinitrogen monoxide gas, and 100. grams of diphosphorus pentoxide gas. The total pressure of the mixture of gases is 1.67 atm. What is the partial pressure of each gas? I have 80. grams of carbon monoxide gas, 55 grams of dinitrogen monoxide gas, and 100. grams of diphosphorus pentoxide gas. The total pressure of the mixture of gases is 1.67 atm. What is the partial pressure of each gas? Dalton’s Law Dalton’s Law 80 g CO / 28 = 2.86 mol 80 g CO / 28 = 2.86 mol 55 g N 2 O / 44 = 1.25 mol 55 g N 2 O / 44 = 1.25 mol 100 g P 2 O 5 / 142 = 0.70 mol 100 g P 2 O 5 / 142 = 0.70 mol TOTAL MOLES = 4.81 moles TOTAL MOLES = 4.81 moles P CO = 2.86/4.81*(1.67) = 0.99 atm P CO = 2.86/4.81*(1.67) = 0.99 atm P N2O = 1.25/4.81*(1.67) = 0.43 atm P N2O = 1.25/4.81*(1.67) = 0.43 atm P P2O5 = 0.70/4.81*(1.67) = 0.24 atm P P2O5 = 0.70/4.81*(1.67) = 0.24 atm