Question
An insulated container has 2.00kg of water at 25◦C to which an unknown amount of ice...
An insulated container has 2.00kg of water at 25◦C to which an unknown
amount of ice at 0◦C is added. The system comes to an equilibrium temperature of
20◦C. The heat capacity for water is 4190 J and the heat of fusion for ice is kg·K
kJ LF =334kg.
(a) Determine the amount of ice that was added to the water.
(b) What is the change in the entropy associated with the ice melting?
(c) What is the change in the entropy of the melted ice water when it changes temperature from zero to the equilibrium temperature, 20◦?
(d) What is the change in the entropy of the hot water when it changes temperature from 25◦C to the equilibrium temperature 20◦?
(e) What is the change in the entropy of the system?
Homework Answers
Answer #1
Not the answer you're looking for?
Similar Questions
You have 1.60 kg of water at 27.0°C in an insulated container of negligible mass. You...
You have 1.60 kg of water at 27.0°C in an insulated container of
negligible mass. You add 0.640 kg of ice that is initially at
-22.6°C. Assume no heat is lost to the surroundings and the mixture
eventually reaches thermal equilibrium. If all of the ice has
melted, what is the final temperature (in °C, round to 2 decimal
places) of the water in the container? Otherwise if some ice
remains, what is the mass of ice (in kg, round...
You have 1.45 kg of water at 27.4°C in an insulated container of negligible mass. You...
You have 1.45 kg of water at 27.4°C in an insulated container of
negligible mass. You add 0.680 kg of ice that is initially at
-22.4°C. Assume no heat is lost to the surroundings and the mixture
eventually reaches thermal equilibrium. If all of the ice has
melted, what is the final temperature (in °C, round to 2
decimal places) of the water in the container? Otherwise
if some ice remains, what is the mass of ice (in kg, round...
An insulated Thermos contains 115 g of water at 78.7 ˚C. You put in a 10.0...
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...
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...
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?
A well-insulated 0.2kg copper bowl contains 0.10kg of ice, both at −10◦ C. A very hot...
A well-insulated 0.2kg copper bowl contains 0.10kg of ice, both
at −10◦ C. A very hot 0.35kg copper cylinder is dropped into it and
the lid quickly closed. The final temperature of the system is
100◦C, with 5g of steam in the container.
(a) How much heat was transferred to the water (in all
phases);
(b) How much to the bowl?
(c) What must have been the original temperature of the
cylinder?
The specific heat of copper is 386 J/kg·K....
You have 1.30 kg of water at 27.6 Degree Celsius in an insulated container of negligible...
You have 1.30 kg of water at 27.6 Degree Celsius in an insulated
container of negligible mass. You add 0.580 kg of ice that is
initially at -21.0 Degree Celsius. Assume no heat is lost to the
surroundings and the mixture eventually reaches thermal
equilibrium. If all of the ice has melted, What is the final
temperature (in Degree Celsius, round to 2 decimal places) of the
water in the container? Otherwise if some ice remains, what is the
mass...
Adding Ice to Water An insulated beaker with negligible mass contains liquid water with a mass...
Adding Ice to Water
An insulated beaker with negligible mass contains liquid water
with a mass of 0.340 kg and a temperature of 66.3 ∘C .
How much ice at a temperature of -17.9 ∘C must be dropped into
the water so that the final temperature of the system will be 22.0
∘C ?
Take the specific heat of liquid water to be 4190 J/kg⋅K , the
specific heat of ice to be 2100 J/kg⋅K , and the heat of...
. 1.0kg of ice at 0oC is added to 10kg of water in a 2.0kg insulated...
. 1.0kg of ice at 0oC is added to 10kg of water in a 2.0kg
insulated aluminum container. The water and aluminum are both
initially at 20oC. Calculate the final equilibrium temperature. (Lf
ice = 3.3x105J/kg), (cAl = 900J/kgoC) In addition find the
following 9. Calculate the heat needed to completely melt a 14kg
bar of gold initially at 20oC. (Tmelt Au = 1064oC), ( cAu =
129J/kgoC), (Lf Au = 6.3x104J/kg)
Chapter 18, Problem 041 (a) Two 58 g ice cubes are dropped into 410 g of...
Chapter 18, Problem 041
(a) Two 58 g ice cubes are dropped into 410 g
of water in a thermally insulated container. If the water is
initially at 20°C, and the ice comes directly from a freezer at
-11°C, what is the final temperature at thermal equilibrium?
(b) What is the final temperature if only one ice
cube is used? The specific heat of water is 4186 J/kg·K. The
specific heat of ice is 2220 J/kg·K. The latent heat of...
ADVERTISEMENT
Need Online Homework Help?
Get Answers For Free
Most questions answered within 1 hours.
ADVERTISEMENT
Active Questions
asked 8 minutes ago
asked 25 minutes ago
asked 39 minutes ago
asked 41 minutes ago
asked 42 minutes ago
asked 51 minutes ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago