Question

A 200 g aluminum calorimeter can contain 500 g of water at 20 C.
A 100 g piece of ice cooled to -20 C is placed in the
calorimeter.

- Find the final temperature of the system, assuming no heat
losses. (Assume that the specific heat of ice is 2.0 kJ/kg K)

- A second 200 g piece of ice at -20 C is added. How much ice
remains in the system after it reaches equilibrium?

- Would your answer to part b be different if both pieces of ice
were added at the same time?

(specific heat of aluminum is 0.9 kJ/kg K and water is 4.18
kJ/kg K)

Answer #1

A 192-g aluminum calorimeter contains 606 g of water at 18° C. A
98-g piece of ice cooled to -18° C is placed in the calorimeter.
(Assume that the specific heat of ice is always 2.02 kJ/kg ·
K.)

An 100-g aluminum calorimeter contains 280 g of water at an
equilibrium temperature of 20°C. A 170-g piece of metal, initially
at 277°C, is added to the calorimeter. The final temperature at
equilibrium is 32°C. Assume there is no external heat exchange. The
specific heats of aluminum and water are 910 J/kg·K and 4190
J/kg·K, respectively. The specific heat of the metal is closest
to:
a) 270 J/kg·K.
b) 240 J/kg·K.
c) 330 J/kg·K.
d) 390 J/kg·K.
e) 360 J/kg·K.

A 0.4-L glass of water at 20°C is to be cooled with ice to 5°C.
The density of water is 1 kg/L, and the specific heat of water at
room temperature is c = 4.18 kJ/kg·°C. The specific heat
of ice at about 0°C is c = 2.11 kJ/kg·°C. The melting
temperature and the heat of fusion of ice at 1 atm are 0°C and
333.7 kJ/kg.
A) Determine how much ice needs to be added to the water, in...

A 100 g aluminum calorimeter contains 250 g of water. The two
substances are in thermal equilibrium at 10°C. Two metallic blocks
are placed in the water. One is a 50 g piece of copper at 82°C. The
other sample has a mass of 78 g and is originally at a temperature
of 100°C. The entire system stabilizes at a final temperature of
20°C. Determine the specific heat of the unknown second sample.

A 500-g aluminum container holds 300 g of water. The water and
aluminum are initially at 40∘C. A 200-g iron block at 0∘C is added
to the water. Assume the specific heat of iron is 450 J/kg⋅∘C, the
specific heat of water 4180 J/kg⋅∘C and the specific heat of
aluminum is 900 J/kg⋅∘C
.
1Determine the final equilibrium temperature.
2.Determine the change in thermal energy of the aluminum
3.Determine the change in thermal energy of the water. 4.
Determine...

A calorimeter contains 82.4 grams of water at 20.9 °C. A 156
-gram piece of an unknown metal is heated to 81.9 °C and dropped
into the water. The entire system eventually reaches 26.6 °C.
Assuming all of the energy gained by the water comes from the
cooling of the metal—no energy loss to the calorimeter or the
surroundings—calculate the specific heat of the metal. The specific
heat of water is 4.18 J/g · °C _____J/g · °C

(a) A student drops two metallic objects into a 120 g steel
container holding 150 g of water at 25◦C. One object is a 200 g
cube of copper that is initially at 85◦C, and the other is a chunk
of aluminum that is initially at 5◦C. To the student’s surprise,
the water reaches a final temperature of 25◦C, precisely where it
started. What is the mass of the aluminum chunk? Specific heats of
water, steel, copper, and aluminum are...

An insulated Thermos contains 115 g of water at 78.7 ˚C. You put
in a 10.0 g ice cube at 0.00 ˚C to form a system of ice +
original water. The specific heat of liquid water is 4190
J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the
net entropy change of the system from then until the system reaches
the final (equilibrium) temperature?

An insulated Thermos contains 113 g of water at 77.3 ˚C. You put
in a 10.3 g ice cube at 0.00 ˚C to form a system of ice + original
water. The specific heat of liquid water is 4190 J/kg•K; and the
heat of fusion of water is 333 kJ/kg. What is the net entropy
change of the system from then until the system reaches the final
(equilibrium) temperature?

An insulated Thermos contains 119 g of water at 75.1 ˚C. You put
in a 9.16 g ice cube at 0.00 ˚C to form a system of ice + original
water. The specific heat of liquid water is 4190 J/kg•K; and the
heat of fusion of water is 333 kJ/kg. What is the net entropy
change of the system from then until the system reaches the final
(equilibrium) temperature?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 1 minute ago

asked 1 minute ago

asked 9 minutes ago

asked 10 minutes ago

asked 13 minutes ago

asked 14 minutes ago

asked 16 minutes ago

asked 22 minutes ago

asked 41 minutes ago

asked 49 minutes ago

asked 50 minutes ago