1. Jeopardy Q $100 Q $100 Q $100 Q $100 Q $100 Q $200 Q $200 Q $200
Ouch! That’s Hot!
Counting Those
Calories
Name that
phase change
What a gas!
NRG definitions
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Final Jeopardy

2. $100 Question from What a Gas
As a beaker of water freezes, is the potential
energy of the water increasing, decreasing or
remaining constant?

3. $100 Answer from What a Gas
Decreasing

4. $200 Question from What a Gas
If a liquid in a closed container is
warmed, its vapor pressure will do this

5. $200 Answer from What a Gas
increase

6. $300 Question from What a Gas
As attractive forces between molecules
increase, one would expect the vapor
pressure of the substance to do this.

7. $300 Answer from What a Gas
decrease

8. $400 Question from What a Gas
100 mL of octane was placed on a hot plate and 100 mL
of water was placed on a second hot plate at the same temperature
Setting. After 30 minutes only 60 mL of octane remained in the beaker
whereas 90 mL of water remained. How do you explain this difference
in final volumes?

9. $400 Answer from What a Gas Octane is a nonpolar molecule with weak
IMF’s and therefore evaporates more easily.

10. $500 Question from What a Gas
Explain how a pressure cooker works.

11. $500 Answer from What a Gas Pressure cookers cook food at a higher
temperature because the water vapor
increases the pressure on the surface of
the liquid in the closed system. This makes
the boiling point of the water increase and the food cooks faster.

12. $100 Question from Ouch! That’s Hot!
When the rate of evaporation of a liquid equals
the rate of condensation in a closed system,
the system has reached this condition.

13. $100 Answer from Ouch! That’s Hot!
Dynamic equilibrium

14. $200 Question from Ouch! That’s Hot!
When water vapor condenses in a closed system, one would expect the temperature of the vapor to do this.

15. $200 Answer from Ouch! That’s Hot!
increase

16. $300 Question from Ouch! That’s Hot!
Given the vapor pressure curves above, name the
substance with the weakest attractive forces

17. $300 Answer from Ouch! That’s Hot!
pentane

18. $400 Question from Ouch! That’s Hot!
Arrange the boiling point of water at the
following locations from highest to lowest:
Top of Mount Washington, N.H.
Top of Hanover High School
Top of Mount Everest

19. $400 Answer from Ouch! That’s Hot!
Top of Hanover High School
Top of Mount Washington
Top of Mount Everest

20. $500 Question from Ouch! That’s Hot!
Go to the board and sketch a potential energy
diagram for a reaction in which the temperature of the surroundings cools. Be sure to label the x and y axes.

21. $500 Answer from Ouch! That’s Hot!

22. $100 Question from NRG definitions
“The temperature at which the vapor
pressure of a liquid is equal to or greater
than the external pressure” defines this term.

23. $100 Answer from NRG definitions
Boiling point

24. $200 Question from NRG definitions
“The amount of heat needed to raise
the temp of an object 1 degree Celsius”
defines this term.

25. $200 Answer from NRG definitions
Heat capacity

26. $300 Question from NRG definitions
A number (including the unit) that represents the amount of heat needed to raise the temperature of 1 gram of water 1 degree celsius.

27. $300 Answer from NRG definitions
4.18 joules or 1 calorie

28. $400 Question from NRG definitions
“The amount of heat needed to raise the
temperature of one gram of a substance
by one degree Celsius” is the definition for
this term.

29. $400 Answer from NRG definitions
Specific heat capacity

30. $500 Question from NRG definitions
The heat content of a system is the definition for this term.

31. $500 Answer from NRG definitions
Enthalpy

32. $100 Question from Counting Those Calories
The sign for the change in enthalpy
in an endothermic reaction

33. $100 Answer from Counting Those Calories
Positive

34. $200 Question from Counting Those Calories
Calculate the enthalpy change in kJ when 45.2 g of steam
at 100°C condenses to water at the same temperature
Δ H vap for H2O = 40.7 kJ/mol

35. $200 Answer from Counting Those Calories
-102 kJ

36. $300 Question from Counting Those Calories
The amount of heat 32.0 g of water
absorbs when it is heated from 25.0°C
to 80.0°C (correct sig figs please).

37. $300 Answer from Counting Those Calories
1,760 calories or 7,360 joules

38. $400 Question from Counting Those Calories
The amount of heat (in kJ) produced when
34.8 g of methane burns
ΔH = kJ/mol
(Report your answer with correct sig
Figs!)

39. $400 Answer from Counting Those Calories
-1940 kJ

40. $500 Question from Counting Those Calories
A 30.0 gram sample of a metal is heated
From 22.0°C to 59.2°C. During the process,
1.0 kJ of energy is absorbed by the metal.
What is the specific heat of the metal?
(correct sig figs please).

41. $500 Answer from Counting Those Calories
0.90 J/g°C

42. $100 Question from Name That Phase Change
The name for the heat released
when a substance changes phase from
gas to liquid.

43. $100 Answer from Name That Phase Change
Heat of Solidification

44. $200 Question from Name that Phase Change
Water freezing - exothermic or
endothermic phase change?

45. $200 Answer from Name That Phase Change
exothermic

46. $300 Question from Name That Phase Change
The opposite of heat of condensation

47. $300 Answer from Name That Phase Change
Heat of vaporization

48. $500 Question from Name That Phase Change
Calculate the heat in kJ associated with
a gram sample of steam at 100.0°C
changing phase to a liquid at 100.0°C.
The heat of vaporization of water is 2,260J/g.
Be sure your answer shows whether the change
is exothermic or endothermic.

49. $500 Answer from Name That Phase Change
-565kJ

50. $400 Question from Name That Phase Change
Watch the demonstration of iodine being heated
at the lab bench. What is the name of this phase change?

51. $400 Answer from Name That Phase Change
sublimation

52. Final Jeopardy
Using the standard heat of formation table in your textbook
on page 530, and the skeleton equation below, calculate the
amount of energy associated with the combustion of 1 mol
of hydrogen sulfide. (∆Hfo for H2S = kJ/mol)
H2S(g) + O2(g) --- H2O(g) + SO2(g)

53. Final Jeopardy Answer
-518 kJ/mol