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WorksheetsPractice Test for Midterm Exam
Total questions: 25
Worksheet time: 3hrs 11mins
There are gaps in the railway tracks to allow tracks to _____________ on a hot day.
burst
contract
expand
ignite
Thermometer is the instrument used to measure ____________________.
Heat energy
Temperature
Specific heat
Specific latent heat
Scale of a thermometer tells how far the ______________rises or goes down.
Mercury
Helium
Nitrogen
Neon
Heat is a form of ________________.
Degree
Scale
Energy
Hotness
Temperature measures how _____ or _____ an object is.
hot, increase
hot, cold
heat, hot
cold, cool
When matter is_________, it will expand an its size or volume become bigger.
Hotted
Cold
Heated
Cooled
Mercury expand and __________ evenly as the temperature changes. This makes it suitable to be used in thermometers.
balance
decreasing
contract
increase
Glass bulb is a part of thermometer which contains ____________________.
Calcium nitrate
Mercury
Acid
Helium
The specific latent heat of vaporization of a substance is the amount of heat needed to change the state of 1kg of the substance from ______________ to ___________ state without any change in temperature.
gas, solid
liquid, gaseous
liquid, solid
solid, gas
The specific latent heat of fusion of a substance is the amount of heat needed to change the state of 1kg of the substance from ______________ to ___________ state without any change in temperature.
solid, gas
solid, liquid
liquid, gas
gas, solid
Covert 85°C to °F
118°F
185°C
118°C
185°F
Covert 35°F into °C
1667°C
166.7°C
1.667°C
16.67°C
Convert 120°C into K
393.93 K
3.93 K
393.15 K
39.15 K
Convert 10°F into K
2609.28 K
260.928 K
26.092 K
2.609 K
Convert 100°C into °F
211 °F
221 °F
212 °F
202 °F
5 g of copper was heated from 20°C to 2=80°C. How much energy was used to heat copper?(c=0.092 cal/g °C)
2.67 cal
26.7 cal
27.6 cal
276 cal
A 155g sample of an unknown substance was heated from 25°C to 40°C. In the process, the substance absorbed 569 calories of energy. What is the specific heat of the substance?
0.24 cal/kg °C
0.18 cal/g °C
0.24 cal/g °C
0.24 cal
How much heat is released when 20g of water at 50°C cools to 25°C? The specific heat of water is 1 cal/g °C.
500 cal
500 J/g
500 J
500 cal/g
How much heat is absorbed by 2kg of water as energy from the fire causes its temperature to change from 10°C to 20°C? (c = 4200 J/kg °C)
74,000 calories
63,000 calories
84,000 Joules
48,000 Joules
The temperature of a sample water increases from 15°C to 30°C as it absorbs 4550 calories of heat. What is the mass of the sample? (specific heat of water is 1.0 cal/g °C)
203.33 J/kg
323.33 g/°C
303.33 g
213.33 kg
How much energy is needed to melt down a 4000 g of mercury? (Lf = 1.14 x 104 J/kg)
45.6 x 104 cal
4.56 x 104 J
45,600 cal
456,000 J
A 5g ice cube is placed on a table. After a while it melts. How much energy was required to melt it? (LF = 80 cal/g °C)
412 cal/g
240 J/kg
400 cal
385 J
Calculate the amount of heat added to 2500 g of gold to change phase from solid to liquid. Heat of fusion for gold is 64500 J/kg.
200,000 joules
121,210 joules
161,250 joules
141, 365 joules
When 1,250 J of heat us added to 4000 g of a metal, it all melts and remains at a constant temperature. What is the heat of fusion of this metal?
0. 414 cal/kg
0.313 J/g
0.212 cal/g
0.18 J/kg
Calculate the mass of a gold bar that absorbed 1, 612, 500 J to change its phase from solid to liquid. Heat of fusion for gold bar is 64500 J/kg.
25 grams
215 kilograms
255 grams
25 kilograms
