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Lakeland Gases Review

Lakeland Gases Review. Click on a question to begin. Question 1. Try Again. Think of PV = nRT for both gases to determine which variables must be the same or different. Try Again. Correct!.

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Lakeland Gases Review

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  1. Lakeland Gases Review

  2. Click on a question to begin

  3. Question 1

  4. Try Again • Think of PV = nRT for both gases to determine which variables must be the same or different Try Again

  5. Correct! • If the two gases have the same pressure, volume and temperature then their number of moles must be the same. This means the same number of particles. Next Question

  6. Question 2

  7. Try Again • As temperature increases the molecules move faster. Try Again

  8. Correct! • As temperature increases the molecules gain more energy and therefore run into the sides of the container holding the gas more often. This causes an increase in pressure. Next Question

  9. Question 3

  10. Try Again • Use the combined gas law to solve for the temperature Try Again

  11. Correct! • P1V1/T1 = P2V2/T2 (3)(1)/288 = (2)(1.50)/T2 Next Question

  12. Question 4

  13. Try Again • Dalton’s Law of Partial Pressure states that the total pressure is equal to the sum of the partial pressures Try Again

  14. Correct! • 4.00 atm + 3.00 atm + 1.00 atm = 8.00 atm Next Question

  15. Question 5

  16. Try Again • This problem requires you to use the ideal gas law. Make sure to convert grams to moles. Try Again

  17. Correct! • PV = nRT (1 atm)V = (576x1/64)(0.0821)(273) Next Question

  18. Question 6

  19. Try Again • Volume and temperature have a direct relationship Try Again

  20. Correct! • As temperature decreases, volume decreases. Next Question

  21. Question 7

  22. Try Again • Use Boyles law to solve the problem. You do not need to convert any units. Try Again

  23. Correct! • P1V1 = P2V2 (600)(200) = (1200)V2 Next Question

  24. Question 8

  25. Try Again • Use Charles Law to solve the problem Try Again

  26. Correct! • V1/T1 = V2/T2 60/546 = V2/273 Next Question

  27. Question 9

  28. Try Again • More heat will increase the speed of the molecules. Try Again

  29. Correct! • An increase in heat causes the molecules to speed up and push out on the sides of the container. This causes an increase in volume. Next Question

  30. Question 10

  31. Try Again • Use the combined gas law Try Again

  32. Correct! • P1V1/T1 = P2V2/T2 • (79)(444)/273 = (1880)(38.7)/T2 Next Question

  33. Question 11

  34. Try Again • Use PV = nRT and be sure to convert grams to moles Try Again

  35. Correct! • PV = nRT (1)V = (156 x 1/44)(0.0821)(273) Next Question

  36. Question 12

  37. Try Again • Pressure and volume are inversely related Try Again

  38. Correct! • As the volume increases, pressure decreases Next Question

  39. Question 13

  40. Try Again • Remember that temperatures need to be in Kelvin when using the gas laws. Try Again

  41. Correct! • As volume increases so does temperature. 200 K to 400 K is a double in temperature, so it also doubles the volume. Next Question

  42. Question 14

  43. Try Again • Think of the ideal gas law. Which variables change with a change in pressure and volume. Try Again

  44. Correct! • The number of molecules remains the same since no gas is able to escape a sealed container. Next Question

  45. Question 15

  46. Try Again • Remember that we use Kelvin for the gas laws. Volume and temperature are inversely proportional. Try Again

  47. Correct! • V1/V2 = T1/T2 40/80 = 293/T2 • so T2 = (80)(293)/(40) Next Question

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