Question

A 50.0 g ice cube at 0.0 degrees C is placed in a lake whose temperature is 14.0 degrees C. Calculate the change in entropy (in joules/Kelvin) of the system as the ice cube comes to thermal equilibrium with the lake. (c for water = 4186 J/kg-K)

Answer #1

A 80 g ice cube at -53°C is placed in a lake whose temperature
is 44°C. Calculate the change in entropy of the cube-lake system as
the ice cube comes to thermal equilibrium with the lake. The
specific heat of ice is 2220 J/kg·K. (Hint: Will the ice cube
affect the temperature of the lake?)

A 49 g ice cube at -69°C is placed in a lake whose temperature
is 32°C. Calculate the change in entropy of the cube-lake system as
the ice cube comes to thermal equilibrium with the lake. The
specific heat of ice is 2220 J/kg·K. (Hint: Will the ice
cube affect the temperature of the lake?)

A 49 g ice cube at -37°C is placed in a lake whose temperature
is 77°C. Calculate the change in entropy of the cube-lake system as
the ice cube comes to thermal equilibrium with the lake. The
specific heat of ice is 2220 J/kg·K. (Hint: Will the ice cube
affect the temperature of the lake?)

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 400 g ice cube at -20 ?C is placed in an aluminum cup whose
initial temperature is 80 ?C . The system comes to an equilibrium
temperature of 20 ?C .
What is the mass of the cup?
Express your answer with the appropriate units.

A 102 g piece of ice at 0.0°C is placed in an insulated
calorimeter of negligible heat capacity containing 100 g of water
at 100°C. Find the entropy change of the universe for this
process?
135 J/K 134 J/K is wrong,

An 11 g ice cube at -12˚C is put into a Thermos flask containing
145 cm3 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 ×
103 J/kg.
and
A 6.0 g ice cube at -21˚C is put into a Thermos...

A cube of ice is taken from the freezer at -6.5 ?C and placed in
a 85-g aluminum calorimeter filled with 300 g of water at room
temperature of 20.0 ?C. The final situation is observed to be all
water at 17.0 ?C. The specific heat of ice is 2100 J/kg?C?, the
specific heat of aluminum is 900 J/kg?C?, the specific heat of
water is is 4186 J/kg?C?, the heat of fusion of water is 333 kJ/Kg.
a)What was the...

A cube of ice is taken from the freezer at -5.5 ∘C and placed in
a 85-g aluminum calorimeter filled with 300 g of water at room
temperature of 20.0 ∘C. The final situation is observed to be all
water at 16.0 ∘C. The specific heat of ice is 2100 J/kg⋅C∘, the
specific heat of aluminum is 900 J/kg⋅C∘, the specific heat of
water is is 4186 J/kg⋅C∘, the heat of fusion of water is 333 kJ/Kg.
What was the...

A 35.0-g cube of ice, initially at 0.0°C, is dropped into 180.0
g of water in an 70.0-g aluminum container, both initially at
35.0°C. What is the final equilibrium temperature? (Specific heat
for aluminum is 900 J/kg⋅°C, the specific heat of water is 4 186
J/kg⋅°C, and Lf = 3.33 × 105 J/kg.)
26.4 °C
17.6 °C
8.79 °C
35.1 °C
30.8 ° C

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