At room conditions, the density of liquid water is about
1 g/mL
18 g/ml
22.4 g/mL
0 g/mL
The boiling point of pure water at standard pressure is
0°C
32°C
100°C
212°C
The freezing point of pure water at standard pressure is
0°C
32°C
100°C
212°C
Which of these phase changes occurs by the removal of energy?
Which of these phase changes occurs by the absorption of energy?
Separate 100 gram masses of iron and liquid water are each allowed to absorb 600 joules of energy. As a result,
the temperature of the water changes more than the temperature of the iron
the temperature of the iron changes more than the temperature of the water
the temperatures of both change by the same amount
neither the water nor the iron experience a temperature change
The temperature would be expected to remain constant during which of the following phase changes?
Use this information to answer the question below: ΔHfus (H2O) = 334 J/g ΔHvap (H2O) = 2260 J/g
How much energy is required to boil 50 grams of water at its boiling point?
100 J
113 000 J
45.2 J
50 J
Use this information to answer the question below: ΔHfus (H2O) = 334 J/g ΔHvap (H2O) = 2260 J/g
How much energy is required to melt 50 grams of ice at its melting point?
16 700 J
113 000 J
6.68 J
50 J
Which of these has the greatest density, assuming standard pressure?
Liquid water at 4°C
Liquid water at 95°C
Ice at -10°C
Steam at 120°C
Refer to the image below when answering this question. Assume standard pressure. As energy is added and one moves from point #5 to point #6, the change taking place is
an increase in the temperature of liquid water
an increase in the density of water
liquid water is becoming steam
ice is melting
Refer to the image below when answering this question. Assume standard pressure. As energy is added and one moves from point #5 to point #6, the temperature
remains constant
increases
decreases
Refer to the image below when answering this question. Assume standard pressure. The temperature at point #6 is
100°C
32°C
0°C
100°F
Refer to the image below when answering this question. Assume standard pressure. At point #2, water would be found as
a liquid only
a solid only
a solid and a liquid
a liquid and a vapor
a vapor only
Refer to the image below when answering this question. Assume standard pressure. As energy is being removed (going right to left), the phase change occuring at point #2 would be
freezing
boiling
condensation
melting
Refer to the image below when answering this question. Assume standard pressure. The temperature at point #1 is
below 0°C
0°C
Between 0°C and 100°C
above 100°C
Refer to the image below when answering this question. Assume standard pressure. The density of water is highest at point
1
2
3
4
5
6
7
Refer to the image below when answering this question. Assume standard pressure. The measure of the energy required to move from point #3 to point #4 on the graph is determined by the
specific heat of liquid water
specific heat of steam
specific heat of ice
heat of fusion of water
heat of vaporization of water
Refer to the image below when answering this question. Assume standard pressure. Which forms of water would be present at point #7?
liquid only
steam only
ice only
liquid and steam
solid and liquid
Refer to the image below when answering this question. Assume standard pressure. The difference in temperature between point #2 and point #6 is
100°C
273°C
32°F
212°F
Refer to the image below when answering this question. Assume standard pressure. Features of this graph support which observations about water?
Which of these is NOT a characteristic of most pure substances, but is true of water?