Question

A large punch bowl holds 3.50 kgkg of lemonade (which is
essentially water) at 22.0 ∘C∘C. A 5.10×10^{−2}-kgkg ice
cube at -10.0 ∘C∘C is placed in the lemonade.

What is the final temperature of the system? Ignore any heat exchange with the bowl or the surroundings.

What is the amount of ice (if any) remaining?

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A large punch bowl holds 3.80 kg of lemonade (which is
essentially water) at 22.0 ∘C. A 6.00×10−2-kg ice cube
at -15.0 ∘C is placed in the lemonade.
What is the final temperature of the system? Ignore any heat
exchange with the bowl or the surroundings. Give your answer in
degrees C.

A large punch bowl holds 3.25 kg of lemonade (which is
essentially water) at 20.0° C. A 1.90-kg ice cube at −10.2°C is
placed in the lemonade. What is the final temperature of the
system, and the amount of ice (if any) remaining? Ignore any heat
exchange with the bowl or the surroundings.

A large punch bowl holds 3.70 kg of lemonade (which is
essentially water) at 25.0 ∘C. A 6.00×10−2-kg ice cube
at -11.0 ∘C is placed in the lemonade.
What is the final temperature of the system? Ignore any heat
exchange with the bowl or the surroundings.
What is the amount of ice (if any) remaining?

A large punch bowl holds 3.30 kg of lemonade (which is
essentially water) at 25.0 ∘C. A 5.50×10^(−2) kg ice cube at -13.0
∘C is placed in the lemonade.
a.What is the final temperature of the system? Ignore any heat
exchange with the bowl or the surroundings. Answer in degree C
b.What is the amount of ice (if any) remaining? Answer in kg

A large punch bowl holds 3.70 kg of lemonade (which is
essentially water) at 25.0 ∘C∘C. A 5.90×10−2-kg ice cube
at -12.0 ∘C is placed in the lemonade. What is the final
temperature of the system? Ignore any heat exchange with the bowl
or the surroundings.

A large punch bowl holds 3.95 kg of lemonade (which is
essentially water) at 20.0

A 9.0×10−2-kg ice cube at 0.0 ∘C is dropped into a
Styrofoam cup holding 0.35 kgkg of water at 10 ∘C∘
A. Find the final temperature of the system. Assume the cup and
the surroundings can be ignored.
B.Find the amount of ice (if any) remaining.
C. Find the initial temperature of the water that would be
enough to just barely melt all of the ice.
Express your answer using two significant figures.

when 50 g of ice at 0 degree c is placed in 400 g of water at 55
degree c, the final temperature is 40 degree c. if we ignore any
exchange of heat to the surroundings, how much heat does it take to
melt 1 g of ice at 0 degree c

A 190 g copper bowl contains 230 g of water, both at 22.0°C. A
very hot 430 g copper cylinder is dropped into the water, causing
the water to boil, with 6.44 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment. (a) How much energy is transferred to the water as
heat? (b) How much to the bowl? (c) What is the original
temperature of the cylinder? The specific heat...

A 110 g copper bowl contains 100 g of water, both at 22.0°C. A
very hot 360 g copper cylinder is dropped into the water, causing
the water to boil, with 7.52 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment. (a) How much energy is transferred to the water as
heat? (b) How much to the bowl? (c) What is the original
temperature of the cylinder? The specific heat...

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