Question

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.

Answer #1

A 40-g block of ice is cooled to
−72°C
and is then added to 590 g of water in an 80-g copper
calorimeter at a temperature of 26°C. Determine the final
temperature of the system consisting of the ice, water, and
calorimeter. (If not all the ice melts, determine how much ice is
left.) Remember that the ice must first warm to 0°C, melt, and then
continue warming as water. (The specific heat of ice is 0.500 cal/g
· °C...

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?

A 40-g block of ice is cooled to −70°C and is then added to 570
g of water in an 80-g copper calorimeter at a temperature of 22°C.
Determine the final temperature of the system consisting of the
ice, water, and calorimeter. (If not all the ice melts, determine
how much ice is left.) Remember that the ice must first warm to
0°C, melt, and then continue warming as water. (The specific heat
of ice is 0.500 cal/g · °C...

A 40-g block of ice is cooled to −76°C and is then added to 570
g of water in an 80-g copper calorimeter at a temperature of 26°C.
Determine the final temperature of the system consisting of the
ice, water, and calorimeter. (If not all the ice melts, determine
how much ice is left.) Remember that the ice must first warm to
0°C, melt, and then continue warming as water. (The specific heat
of ice is 0.500 cal/g · °C...

How many grams of ice at 0.0 degress C must be added to 26.2 g
of water at 21 deg C to give a final temp in the flask of 0.5 deg
C?

A 1.70-kg piece of aluminum that has a temperature of −147 °C is
added to 1.00 kg of water that has a temperature of 3.1 °C. At
equilibrium the temperature is 0.0°C. Assuming that the heat
exchanged with the container and the surroundings is negligible,
determine the mass of water that has been frozen into ice.

Ice of mass 52.5 g at -10.7° C is added to 220 g of water at
15.4° C in a 110 g glass container of specific heat 0.200 cal/g-°C
at an initial temperature of 25.1° C. Find the final temperature of
the system.

Ice of mass 46.5 g at -10.5° C is added to 214 g of water at
14.4° C in a 110 g glass container of specific heat 0.200 cal/g-°C
at an initial temperature of 23.7° C. Find the final temperature of
the system.
°C

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 quantity of ice at 0.0 °C was added to 33.6 g of water at 41.0
°C to give water at 0.0 °C. How much ice was added? The heat of
fusion of water is 6.01 kJ/mol, and the specific heat is 4.18
J/(g•°C). ______ grams

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