Question

A 11 kg block of ice at -15 °C is added to an insulated container partially filled with 12 kg of water at 20 °C.

Given: Cw = 4186 J/kg. °C; Cice = 2220 J/kg. °C, L= 3.34x10 J/kg

(a) Determine the final state of the mixture. Explain your answer.

Based on your answer in (a),

calculate either one (1) of the following: the mass of ice that melts. the final temperature of the system.

(c) Based on your answer in Q4(b), the system is then heated to 110°C. Assuming all water vaporizes, calculate the total energy of the system. Given: Ly = 2.26x100 J/kg, Csteam = 2.01x10' J/kg. °C

Answer #1

Q4 A ZZ kg block of ice at -15 °C is added to an insulated
container partially filled with 12 kg of water at 20 °C.
(Where ZZ = random number as shown in the attachment file. Note
that if you do not use the proper numbers, your answer will be
considered wrong.) Given: cw = 4186 J/kg.°C; cice = 2220 J/kg.°C,
Lf = 3.34×10 5 J/kg
(a) Determine the final state of the mixture.
Explain your answer.
(b) Based...

A 0.66300.6630 kg ice cube at −12.40−12.40 °C is placed inside a
rigid, thermally isolated chamber containing steam at 365.0365.0
°C. Later, you notice that the ice cube has completely melted into
a puddle of water. The specific heats of ice, water, and steam are
?ice=2093 J/(kg·∘C),cice=2093 J/(kg·∘C), ?water=4186
J/(kg·∘C),cwater=4186 J/(kg·∘C), and ?steam=2009
J/(kg·∘C),csteam=2009 J/(kg·∘C), respectively.
If the chamber initially contained 6.1906.190 moles of steam
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You have 1.60 kg of water at 27.0°C in an insulated container of
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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 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...

(a) An insulated container holds 2.0 kg of water at 303 K. You
add 0.15 kg of ice at 273 K. When the mixture comes to equilibrium,
what is its final temperature?
cwater = 4186 J/kg K
Lfusion ice/water = 3.34 x 105 J/kg
(b) An insulated container holds 2.0 kg of water at 303 K. You
add a piece of copper with mass 0.10 kg. The combination comes to a
final temperature of 307 K. What was the original...

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
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What is the minimum amount of heat, in Joules, needed to fully
convert a 1-kg block of ice at 250 K to steam?
cice = 2090 J/kg-°C , cwater = 4186 J/kg-°C ,
csteam = 2010 J/kg-°C,
Lfushion-water 3.33x105 J/kg,
Lvaporization-water = 2.26x106
J/kg

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
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equilibrium. If all of the ice has melted, What is the final
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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...

A 24 g block of ice is cooled to −63◦C. It is added
to 572 g of water in a 98 g copper calorimeter at a temperature of
30◦C.
Find the final temperature. The specific heat of copper is 387
J/kg ·◦C and of ice is 2090 J/kg ·◦C. The
latent heat of fusion of water is 3.33 × 105 J/kg and its specific
heat is 4186 J/kg·◦C.
Answer in units of ◦C.

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