1. Given a gas is at 5 atm and 14 L, what is the volume of the gas when pressure changes to 4 atm? 2. Given a gas is at 10 atm and 24 L, what is the volume of the gas when pressure changes to 7 atm? 3. Given a gas is at 7 atm and 23 L, what is the volume of the gas when pressure changes to 4 atm? 4. A gas at 20^circ C has a pressure of 1 atm. If the temperature is increased to 125^circ C what will be the new pressure? 5. A sealed container with a gas initially at 320 K has a pressure of 2 atm . If the temperature rises to 470 K, what will be the new pressure? 6. A gas occupies 500 mLat 57^circ C . If heated to 127^circ C while keeping pressure constant, what will be its new volume? 7. In a laboratory experiment,a gas is heated from 15^circ C to 100^circ C in a rigid container. If the initial pressure was 1.5 atm , what will be the final pressure? 8. Given a gas is at 2 atm and 9 L, what is the volume of the gas when pressure changes to 1 atm? 9. Given a gas is at 3 atm and 15 L, what is the pressure of the gas when volume changes to 12 L? 10. Given a gas is at 16 L and 112circ C , what is the temperature of the gas when volume changes to 25 L? 11. Given a gas is at 12 L and 260 K, what is the temperature of the gas when volume changes to 3 L? 12. Given a gas is at 9 L and 1circ C what is the volume of the gas when temperature changes to 125^circ C 13. Given a gas is at 6 L and 262 K, what is the volume of the gas when temperature changes to 289 K? 14. Given a gas is at 24 L and 346 K, what is the volume of the gas when temperature changes to 336 K? 15. Given a gas is at 9 L and 9 mol, what is the number of moles of the gas when volume changes to 7 L? 16. Given a gas is at 14 L and 9 mol, what is the number of moles of the gas when volume changes to 4 L? 17. Given a gas is at 21 L and 8 mol, what is the volume of the gas when the number of moles changes to 9 mol? 18. Given a gas is at 10 L and 9 mol, what is the volume of the gas when the number of moles changes to 7 mol? 19. At what temperature will 2.0 moles of an ideal gas have a pressure of 2.0 atm in a 10.0 L container? (R=0.0821Lcdot atm/molcdot K)

1. Using Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure when temperature is held constant, we can calculate the new volume of the gas when the pressure changes. The formula is P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume. Plugging in the given values, we get 5 atm * 14 L = 4 atm * V2. Solving for V2, we get V2 = 17.5 L.<br /><br />2. Using Boyle's Law again, we can calculate the new volume of the gas when the pressure changes. Plugging in the given values, we get 10 atm * 24 L = 7 atm * V2. Solving for V2, we get V2 = 34.29 L.<br /><br />3. Using Boyle's Law, we can calculate the new volume of the gas when the pressure changes. Plugging in the given values, we get 7 atm * 23 L = 4 atm * V2. Solving for V2, we get V2 = 41.25 L.<br /><br />4. Using Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its temperature when volume is held constant, we can calculate the new pressure of the gas when the temperature changes. The formula is P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature. Plugging in the given values, we get 1 atm / (273.15 + 20) K = P2 / (273.15 + 125) K. Solving for P2, we get P2 = 1.47 atm.<br /><br />5. Using Gay-Lussac's Law, we can calculate the new pressure of the gas when the temperature changes. Plugging in the given values, we get 2 atm / 320 K = P2 / 470 K. Solving for P2, we get P2 = 2.94 atm.<br /><br />6. Using Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant, we can calculate the new volume of the gas when the temperature changes. The formula is V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature. Plugging in the given values, we get 500 mL / (273.15 + 57) K = V2 / (273.15 + 127) K. Solving for V2, we get V2 = 805.56 mL.<br /><br />7. Using Gay-Lussac's Law, we can calculate the new pressure of the gas when the temperature changes. Plugging in the given values, we get 1.5 atm / (273.15 + 15) K = P2 / (273.15 + 100) K. Solving for P2, we get P2 = 2.04 atm.<br /><br />8. Using Boyle's Law, we can calculate the new volume of the gas when the pressure changes. Plugging in the given values, we get 2 atm * 9 L = 1 atm * V2. Solving for V2, we get V2 = 18 L.<br /><br />9. Using Boyle's Law, we can calculate the new pressure of the gas when the volume changes. Plugging in the given values, we get 3 atm * 15 L = P2 * 12 L. Solving for P2, we get P2 = 3.75 atm.<br /><br />10. Using Charles's Law, we can calculate the new temperature of the gas when the volume changes. Plugging in the given values, we get 16 L / (273.15 + 112) K = 25 L / T2. Solving for T2, we get T2 = 343.15 K.<br /><br />11. Using Charles's Law, we can calculate the new temperature of the gas when the volume changes. Plugging in the given values, we get 12 L / 260 K = 3 L / T2. Solving for T2, we get T2 = 39.23 K.<br /><br />12. Using Charles's Law, we can calculate the new volume of the gas when the temperature changes. Plugging in the given values, we get 9 L / (273.15 + 1) K = V2 / (273.15 + 125) K. Solving for V2, we get V2 = 11.11 L.<br /><br />13. Using Charles's Law, we can calculate the new volume of the gas when the temperature changes. Plugging in the given values, we get 6 L / 262 K =