Question

8. A 180 g block of copper heated to 120 degrees Celsius dropped
into a 360 g aluminum calorimeter container

containing 440 g of water. If the initial temperature of the
calorimeter and the water is 20 °C,

what is the final equilibrium temperature of the system?

9. 25 g steam at 110 °C is added temperature of the resulting
water 100 g of ice at -10 °C in an

insulated container. What is the final temperature of the resulting
water?

Answer #1

a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g
degrees Celsius) is heated to 82.4 degrees Celsius and dropped into
a calorimeter containing water (specific heat capacity of water is
4.18 J/g degrees Celsius) initially at 22.3 degrees Celsius. The
final temperature of the water is 24.98 degrees Celsius. Calculate
the mass of water in the calorimeter.

A 100-gram metal block is initially heated to 100 degrees
Celsius. The copper block is then placed in 200-grams of water at
20 degrees Celsius. The block and the water are allowed to come to
thermal equilibrium and reach a temperature of 23.52 degrees
Celsius. a.) What is the change in temperature of the block and the
water? b.) If the specific heat of water is 4.184 J/g C, what is
the heat gained by the water? c.) What is...

500 grams of ice at -16 degrees Celsius are dropped into a
calorimeter containing 1000 grams of water at 20 degrees Celsius.
The calorimeter can is of copper and has a mass of 278 grams.
Compute the final temperature of the system, assuming no heat
losses.

An insulated aluminum calorimeter vessel of 150 g mass contains
300 g of liquid nitrogen boiling at 77 K. A metal block at an
initial temperature of 303 K is dropped into the liquid nitrogen.
It boils away 15.8 g of nitrogen in reaching thermal equilibrium.
The block is then withdrawn from the nitrogen and quickly
transferred to a second insulated copper calorimeter vessel of 200
g mass containing 500 g of water at 30.1 degrees celsius. The block
coolds...

A
47.5 block of an unknown metal is heated in a hot water bath to 100
degrees Celsius. When the block is placed in an insulated vessel
containing 130.0 g of water at 25.0 degrees Celsius, the final
temperature is 28.0 degrees Celsius. Determine the specific heat of
the unknown metal. The Cs for water is 4.18 J/g degrees
Celsius.

A 200 g block of copper at a temperature of 75°C is dropped into
650 g of water at 35°C. The water is contained in a 400 g glass
container. What is the final temperature of the mixture?

A sample of copper weighing 12.0g is heated to 100.0 degrees
celsius and then placed 50.0 mL of water at 26.5 degrees celsius.
What will the final temperature of the water be?

A 190.0 g piece of lead is heated to 87 °C and then dropped into
a calorimeter containing 679.0 g of water that initially is at
20.0°C.
Neglecting the heat capacity of the container, find the final
equilibrium temperature, in °C, of the lead and water.
--Show all work please! Thank you

(a) A student drops two metallic objects into a 120 g steel
container holding 150 g of water at 25◦C. One object is a 200 g
cube of copper that is initially at 85◦C, and the other is a chunk
of aluminum that is initially at 5◦C. To the student’s surprise,
the water reaches a final temperature of 25◦C, precisely where it
started. What is the mass of the aluminum chunk? Specific heats of
water, steel, copper, and aluminum are...

100g of ice at 0 degrees celsius is held in a copper pan (400g).
500g of water at 50 degrees celsius is added. What is the final
temperature of the system?

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