1. Gas Laws REVIEW GAME

2. 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

3. 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

4. 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 = 1.045 mol 20.9 g Ne / 20 = 1.045 mol P(19) = 1.045(0.0821)(254) P(19) = 1.045(0.0821)(254) P = 1.2 atm P = 1.2 atm

5. 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 / 251 4.45 / 287 = V 2 / 251 V 2 = 3.9 L V 2 = 3.9 L

6. Question 5 A gas occupies a volume of 0.65 L at 118.3 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 118.3 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 118.3 kPa x (1 atm/101.325 kPa) = 1.17 atm 118.3 kPa x (1 atm/101.325 kPa) = 1.17 atm 1.17(0.65)/273 = 2.5V 2 /323 1.17(0.65)/273 = 2.5V 2 /323 V 2 = 0.36 L V 2 = 0.36 L

7. 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

8. Question 7 When a container is filled with 6.000 grams of H 2, 64.00 grams of O 2, and 28.00 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 6.000 grams of H 2, 64.00 grams of O 2, and 28.00 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 3+2+1 = 6 total moles 3+2+1 = 6 total moles P O2 = 2/6(5412) = 1804 kPa P O2 = 2/6(5412) = 1804 kPa

9. 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

10. 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

11. 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 / 283 185/458 = P 2 / 283 P 2 = 114 kPa P 2 = 114 kPa

12. 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

13. 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 300.0 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 300.0 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) 0.0171 mol N 2 0.0171 mol N 2

14. 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 / 101.325 kPa) = 36.85 psi 254 kPa ( 14.7psi / 101.325 kPa) = 36.85 psi 36.85(125) = 1.78V 36.85(125) = 1.78V V = 2590 mL V = 2590 mL

15. 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 = 24 + 48 + P o2 95 = 24 + 48 + P o2 P o2 = 23 kPa P o2 = 23 kPa

16. 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 (101.325 kPa / 1atm ) = 124.6 kPa 1.23 atm (101.325 kPa / 1atm ) = 124.6 kPa 124.6 kPa = P gas + 10.62 124.6 kPa = P gas + 10.62 P gas = 113.98 kPa P gas = 113.98 kPa 113.98(590) / 320 = 101.325(V 2 ) / 298 113.98(590) / 320 = 101.325(V 2 ) / 298 620 mL 620 mL

17. 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

18. 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

19. Question 17 93.0 mL of O 2 gas is collected over water at 0.930 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 0.930 atm and 10.0°C. What would be the volume of this dry gas at standard conditions? Dalton and Combined Dalton and Combined 0.930 atm x (101.325 kPa / 1atm) = 94.23 kPa 0.930 atm x (101.325 kPa / 1atm) = 94.23 kPa 94.23 kPa = P gas + 1.2281 94.23 kPa = P gas + 1.2281 P gas = 93 kPa P gas = 93 kPa 93(93)/283 = 101.325V 2 /273 93(93)/283 = 101.325V 2 /273 V 2 = 82.3 mL V 2 = 82.3 mL

20. 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 / 28 6.2 L 6.2 L

21. 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

22. 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

23. 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

24. 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

25. 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 /348 150/298 = V 2 /348 V 2 = 175 mL V 2 = 175 mL

26. 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

27. 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

28. Question 26 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? 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

29. 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 /323 150/300 = P 2 /323 160 kPa 160 kPa

30. 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

31. 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 (101.325 kPa/760 mmHg) = 106.7 kPa 800 mmHg x (101.325 kPa/760 mmHg) = 106.7 kPa 106.7 = P gas + 2.0644 106.7 = P gas + 2.0644 104.6 kPa 104.6 kPa 104.6(100)/291 = 101.325V 2 /273 104.6(100)/291 = 101.325V 2 /273 V 2 = 97 mL V 2 = 97 mL

32. 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

33. 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