Question

An 11 g ice cube at -12˚C is put into a Thermos flask containing
145 cm^{3} of water at 24˚C. By how much has the entropy of
the cube-water system changed when a final equilibrium state is
reached? The specific heat of ice is 2200 J/kg K and that of liquid
water is 4187 J/kg K. The heat of fusion of water is 333 ×
10^{3} J/kg.

and

A 6.0 g ice cube at -21˚C is put into a Thermos flask containing
120 cm^{3} of water at 24˚C. By how much has the entropy of
the cube-water system changed when a final equilibrium state is
reached? The specific heat of ice is 2200 J/kg K and that of liquid
water is 4187 J/kg K. The heat of fusion of water is 333 ×
10^{3} J/kg.

Answer #1

An 10 g ice cube at -13˚C is put into a Thermos flask containing
115 cm3 of water at 20˚C. By how much has the entropy of
the cube-water system changed when a final equilibrium state is
reached? The specific heat of ice is 2200 J/kg K and that of liquid
water is 4187 J/kg K. The heat of fusion of water is 333 ×
103 J/kg.

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?

You decide to put a 40.0 g ice cube at -10.0°C into a well
insulated coffee cup (of negligible heat capacity)
containing of water at 5.0°C. When equilibrium is
reached, how much of the ice will have melted? The specific heat of
ice is 2090 J/kg ∙ K, that of water is 4186 J/kg ∙ K, and the
latent heat of fusion of water is 33.5 × 104 J/kg.

A 25 g ice cube at -15.0oC is placed in 169 g of
water at 48.0oC. Find the final temperature of the
system when equilibrium is reached. Ignore the heat capacity of the
container and assume this is in a calorimeter, i.e. the system is
thermally insulated from the surroundings. Give your answer in
oC with 3 significant figures.
Specific heat of ice: 2.090 J/g K
Specific heat of water: 4.186 J/g K
Latent heat of fusion for water: 333...

A 16 g ice cube at -15.0oC is placed in 140 g of
water at 48.0oC. Find the final temperature of the
system when equilibrium is reached. Ignore the heat capacity of the
container and assume this is in a calorimeter, i.e. the system is
thermally insulated from the surroundings. Give your answer in
oC with 3 significant figures.
Specific heat of ice: 2.090 J/g K
Specific heat of water: 4.186 J/g K
Latent heat of fusion for water: 333...

I place an ice cube with a mass of 0.223 kg and a temperature of
−35°C is placed into an insulated aluminum
container with a mass of 0.553 kg containing 0.452 kg of water. The
water and the container are initially in thermal equilibrium at a
temperature of 27°C. Assuming that no heat enters
or leaves the system, what will the final temperature of the system
be when it reaches equilibrium, and how much ice will be in the
container...

( A = 18, B = 93). A (10.0+A) g ice cube at -15.0oC
is placed in (125+B) g of water at 48.0oC. Find the
final temperature of the system when equilibrium is reached. Ignore
the heat capacity of the container and assume this is in a
calorimeter, i.e. the system is thermally insulated from the
surroundings. Give your answer in oC with 3 significant
figures.
Specific heat of ice: 2.090 J/g K
Specific heat of water: 4.186 J/g K...

A = 13 B = 27
A (10.0+A) g ice cube at -15.0oC is placed in (125+B)
g of water at 48.0oC. Find the final temperature of the
system when equilibrium is reached. Ignore the heat capacity of the
container and assume this is in a calorimeter, i.e. the system is
thermally insulated from the surroundings. Give your answer
inoC with 3 significant figures.
Specific heat of ice: 2.090 J/g K Specific heat of water: 4.186
J/g K Latent heat...

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