The pressure exerted by evaporated liquid particles on the surface of the liquid is called:

1. The pressure exerted by evaporated liquid particles on the surface of the liquid is called:

2. Vapor pressure

3. Which state of matter has the least attraction between particles?

4. gas

5. The process in which particles turn from liquid to vapor from the surface of the liquid is called: __________________

6. evaporation

7. How can a liquid be made to boil below its boiling point?

8. Lower the atmospheric pressure

9. Two ways that a liquid could be made to boil above its boiling point are:

10. Raise the atmospheric pressure • Add a solute

11. Which state of matter below has the highest potential energy? a. Solid b. Liquid c. Gas d. aqueous

12. C. Gas

13. Which state below exhibits the highest entropy? • a. Solid b. Liquid c. Gas d. aqueous

14. C. Gas

15. Systems in nature tend to go favor __________ energy and __________ entropy.

16. Systems in nature tend to go favor __low________ energy and __high________ entropy

17. The normal melting point of this substance is approximately:

18. 100°C

19. At 400°C and 1.50atm, this substance is a _________.

20. Liquid

21. The phase change that occurs as the pressure is raised from 0.25atm to 1.25atm at 400°C is called ________. The sign of ΔH for this phase change is _________;.

22. Condensation, negative

23. The phase change that occurs as the temperature is raised from -100°C to 200°C at 1.25atm is called ________. The sign of ΔH for this phase change is _________.

24. Melting; positive

25. C2H5OH(l) + 3 O2(g)  2 CO2(g) + 3 H2O (g)ΔH = -1418 kJ Is energy absorbed or released in the reaction above?

26. released

27. C2H5OH(l) + 3 O2(g)  2 CO2(g) + 3 H2O (g)ΔH = -1418 kJ • Does entropy increase or decrease in the reaction above? • What is the sign of ΔS?

28. increase

29. C2H5OH(l) + 3 O2(g)  2 CO2(g) + 3 H2O (g)ΔH = -1418 kJ • Under what temperature conditions will this reaction be spontaneous?

30. Any temperature

31. Which sample below has the highest average kinetic energy? • A. Liquid water at 100°C • B. Steam at 100°C • C. Solid lead at 250°C • D. Gaseous nitrogen at 23°C

32. C. Solid lead at 250°C

33. Which sample below has the highest potential energy? • A. Liquid water at 100°C • B. Steam at 100°C • C. Solid lead at 450°C • D. liquid nitrogen at -100°C

34. B – steam at 100°C

35. Which substance below would have the lowest specific heat capacity? a. Iron b. SiO2 c. water

36. A. Iron

37. The beaker became warm when the precipitate formed from the supersaturated solution we made. • The sign of ΔH for this process is _________. • The sign of ΔS for this process is ___________.

38. ΔH is negative. • ΔS is negative.

39. m x sh x ΔT = m x sh x ΔT metal water • While finding the specific heat of a metal in lab, a student takes the initial temperature of the water in the calorimeter without letting the thermometer cool down from measuring the temperature of the metal. • This would make the calculated specific heat of the metal too _________.

40. Too low.

41. m x sh x ΔT = m x sh x ΔT metal water • While finding the specific heat of a metal in lab, a student accidentally spilled some of the water from the calorimeter, after he had already recorded its mass. • This would make the calculated specific heat of the metal too _________.

42. Too low

43. m x sh x ΔT = m x sh x ΔT metal water • While finding the specific heat of a metal in lab, a student forgets to zero the balance with the cup on it. • This would make the calculated specific heat of the metal too _________.

44. Too high

45. Which segment(s) on the graph show a change in kinetic energy?

46. Segments AB, CD, and EF

47. The process that occurs moving from point E to point D is called _____________. The sign of ΔH for this process is _______________.

48. Condensation; negative

49. The melting point of the substance could be determined at points _____ or ______ on the graph below.

50. B or C