15-2

**Gas Equations Worksheet** //<---Previous Assignment - Next Assignment--->media type="custom" key="12534212"// **__Instructions__**
 * __Time Length__ **
 * 3 Days

//On a new wiki titled __15-2 Gas Equations Worksheet__ Show work for 1 random question from each section and just give the answers to the rest.//

// **__Worksheet__** //
 * Boyle's Law**

Standard pressure = 1atm=760 mm Hg = 101.3 kPa

Determine the new volume for each of these pressure changes. Determine the new pressure for each of these volume changes. Determine the new volume for each of these temperature changes. //Don’t forget to use Kelvin temperatures! add 273 to Celcius to get Kelvin! =) Standard temperature is 0// ° C Determine the new temperature for each of these volume changes. //Don’t forget to use Kelvin temperatures!// Determine the pressure of gas 1. total pressure = gas 1 + gas 2 + gas 3 Determine the unknown quantity for each problem. Staple your work to the back. Determine the missing data. Assume all gases are dry. Staple your work to the back. //Don’t forget to use Kelvin temperatures. ST = Standard Temperature = 273 K. SP = Standard Pressure =1 atm//
 * 1. 100.0 mL at 780.0 mm Hg to standard pressure
 * 2. 250.0 mL at standard pressure to 740.0 mm Hg
 * 3. 25.0 mL at standard pressure to 600.0 mm Hg
 * 4. 750.0 mL at 700.0 torr to 800.0 torr
 * 5. 45.0 mL at 1.045 atm to 1.050 atm
 * 6. 130.0 mL at 785 torr to 140.0 mL
 * 7. 65.5 mL at 680.0 torr to 40.0 mL
 * 8. 250.0 mL at standard pressure to 225 mL
 * 9. 16.8 L at 1.000 atm to 15.0 L
 * 10. 22.4 L at 0.853 atm to 24.0 L
 * Charles’ Law**
 * 11. 125 mL at 25.0 ° C to standard temperature
 * 12. 310.0 mL at 58 ° C to 15.0 ° C
 * 13. 20.0 mL at 33.0 ° C to 57.0 ° C
 * 14. 350.0 mL at -30.0 ° C to standard temperature
 * 15. 2.0 L at -45.5 ° C to standard temperature
 * 16. 85.0 mL at 14 ° C to 74.0 mL
 * 17. 39.0 mL at 28 ° C to 30.0 mL
 * 18. 100.0 mL at 0.0 ° C to 35 mL
 * 19. 5.00 mL at 5.0 ° C to 5.5 mL
 * 20. 10.0 L at 10.0 ° C to 5.00 L
 * Dalton’s Law**
 * 21. Total pressure = 440 mm Hg, Gas 2 = 73 mm Hg, Gas 3 = 300 mm Hg
 * 22. Total pressure = 720 mm Hg, Gas 2 = 93 mm Hg, Gas 3 = 330 mm Hg
 * 23. Total pressure = 9000 mm Hg, Gas 2 = 89 mm Hg, Gas 3 = 3000 mm Hg
 * 24. Total pressure = 760 mm Hg, Gas 2 = 4 mm Hg, Gas 3 = 240 mm Hg
 * 25. Total pressure = 435 mm Hg, Gas 2 = 3 mm Hg, Gas 3 = 145 mm Hg
 * Ideal Gas Law**
 * 26. What pressure will be exerted from 0.50 moles of a gas contained in a 1.00 L flask at 25.0 ° C?
 * 27. Find the number of moles of a gas if 1.0 L of it at 15.0 ° C has a pressure of 5 atm.
 * 28. What volume will be occupied by 1.35 moles of a gas at 100 ° C and 2.58 atm of pressure?
 * 29. Calculate the value of the gas constant (R) using STP, one mole of gas, and the volume for one mole of a gas (22.4 L).
 * 30. What will be the pressure of 0.010 mol of oxygen gas in a 4.5 L flask at a temperature of 104 ° C?
 * Ideal Gas Law (pt 2)**


 * |||||| **initial**  ||   ||||||  **final**  ||   ||
 * || **V**  ||  **P**  ||  **T**  || **n** ||  **V**  ||  **P**  ||  **T**  || n ||
 * **31** ||  80.0 mL  ||  720.0 torr  ||  27 ° C  || 1 mol ||   ||  740.0 torr  ||  0.0 ° C  || 1 mol ||
 * **32** ||  36 mL  ||  SP  ||  ST  || 1 mol ||   ||  5 atm  ||  35.0 ° C  || 1 mol ||
 * **33** ||  2.0 L  ||  7 atm  ||  -45 ° C  || 1 mol ||   ||  SP  ||  ST  || 1 mol ||
 * **34** ||  4.50 L  ||  1.035 atm  ||  375 K  || 1 mol ||   ||  1.100 atm  ||  350. K  || 1 mol ||
 * **35** ||   ||  745 mm Hg  ||  30.0 ° C  || 1 mol ||  185 mL  ||  685 mm Hg  ||  28 ° C  || 1 mol ||