Question

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.

Answer #1

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...

A small ice cube (initially at -5.00 degrees Celsius) is placed
in a calorimeter along with 750.0 grams of water (at 45.00 degrees
Celsius) and a 250.0 gram piece of copper (at 100.00 degrees
Celsius). The system comes to thermal equilibrium at 43.34 degrees
Celsius. What is the mass of the ice cube?

200
grams of water at 65 degrees celsius are mixed with 40 grams of ice
at 0 degrees celsius in a 50 gram aluminum calorimeter cup at 25
degrees celsius. What is the final state of the system (all
substances and temperatures?)

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.

There is 300 grams of water in the 200-gram calorimeter cup
(inner can). Both are at room temperature of 20 degrees Celsius. A
100-gram metal sample with an initial temperature of 90 degrees
Celsius is placed in the calorimeter resulting. The resulting final
temperature of the system is 30 degrees Celsius. If the calorimeter
can has a specific heat of 0.2 cal/g-C degree, determine the
specific heat of the metal sample

A copper calorimeter can with mass 0.860 kgcontains 0.185 kg of
water and 0.020 kg of ice in thermal equilibrium at atmospheric
pressure.
If 0.775 kg of lead at a temperature of 255 ∘C is dropped into
the can, what is the final temperature of the system? (Assume no
heat is lost to the surroundings.)
Express your answer in degrees Celsius to three
significant figures.

Imagine 25 grams of ice at -5.0 degrees Celsius and 0.12 liters
of water at 33 degrees Celsius. If we mix them in an ideal
calorimeter, what equilibrium temperature should we expect?

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...

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?

Some ice at -15 degrees celcius with a mass of 0.45 kg is
dropped into a highly insulated cup (no heat flows into or out of
cup) with 3.0 kg water that is at 20 degrees celcius.
Determine if all the ice has melted
What if the final temperature of the water in the cup?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 17 minutes ago

asked 32 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 53 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago