Question

A 39.2 g cube of ice, initially at 0.0 °C, is dropped into 220 g of water in an 80-g aluminum container. The water is initially at 35 °C and the aluminum container is initially at 25 °C. Remember to take in to account the melting of the ice. What is the final equilibrium temperature in °C?

Answer #1

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

(a) Two 64 g ice cubes are dropped into 278 g of water in a
thermally insulated container. If the water is initially at 25°C,
and the ice comes directly from a freezer at −15°C, what is the
final temperature at thermal equilibrium? (in celcius)
(b) What is the final temperature if only one ice cube is used?
(in celcius)

A 46.5 g ice cube, initially at 0°C, is dropped into a Styrofoam
cup containing 348 g of water, initially at 21.4°C. What is the
final temperature of the water, if no heat is transferred to the
Styrofoam or the surroundings?

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere).
1.Determine the final (equilibrium) temperature of the
icewater mixture.
2. Determine the phase (ie., liquid or solid) corresponding to
the...

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...

Ice with a mass of 52 g originally at 0.0 deg. C is added to 450
g of water originally at 80. deg. C. Determine the final
temperature once all the ice melts and all the water reaches
thermal equilibrium. Assume that no heat is exchanged with the
container.

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...

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere)
a) Describe what happens to each ice cube (and why)
b) If (Lv)Nitrogen =48 kcal/kg, (LF)Nitrogen = 6.1 kcal/kg,
and...

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere)
a) Describe what happens to each ice cube (and why)
b) If (Lv)Nitrogen =48 kcal/kg, (LF)Nitrogen = 6.1 kcal/kg,
and...

A 112-g cube of ice at 0°C is dropped into 1.0 kg of water that
was originally at 82°C. What is the final temperature of the water
after the ice has melted?
in C

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