Question

A 50 gram piece of copper at 200°C is placed in 100 grams of water at 25°C. Assuming no loss of heat to the surroundings, determine the final temperature of the water and copper.

Answer #1

**specific heat capacity of copper = 0.385
J/g.oC**

**specific heat capacity of water = 4.184
J/g.oC**

**Let us denote Cu by symbol 1 and water by symbol
2**

**m1 = 50.0 g**

**T1 = 200.0 oC**

**C1 = 0.385 J/goC**

**m2 = 100.0 g**

**T2 = 25.0 oC**

**C2 = 4.184 J/goC**

**T = to be calculated**

**Let the final temperature be T oC**

**use:**

**heat gained by 2 = heat lost by 1**

**m2*C2*(T-T2) = m1*C1*(T1-T)**

**100.0*4.184*(T-25.0) = 50.0*0.385*(200.0-T)**

**418.4*(T-25.0) = 19.25*(200.0-T)**

**418.4*T -10460 = 3850 - 19.25*T)**

**T= 32.7 oC**

**Answer: 32.7 oC**

Two 50 gram ice cubes are dropped into 200 grams of water in a
class. 1.) if the water was initially at a temperature of 25
degrees C, and if the ice came directly from a freezer operating at
-15 degrees C, what will be the final temperature of the drink? The
specific heat of ice is about 0.50 cal/(gram degree C) in this
temperature range, and the heat required to melt ice to water is
about 80 cal/gram. 2.)...

A calorimeter contains 82.4 grams of water at 20.9 °C. A 156
-gram piece of an unknown metal is heated to 81.9 °C and dropped
into the water. The entire system eventually reaches 26.6 °C.
Assuming all of the energy gained by the water comes from the
cooling of the metal—no energy loss to the calorimeter or the
surroundings—calculate the specific heat of the metal. The specific
heat of water is 4.18 J/g · °C _____J/g · °C

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 401−g piece of copper tubing is heated to 89.5°C and placed in
an insulated vessel containing 159 g of water at 22.8°C. Assuming
no loss of water and a heat capacity for the vessel of 10.0 J/°C,
what is the final temperature of the system (c of copper = 0.387
J/g·°C)?

A 404−g piece of copper tubing is heated to 89.5°C and placed in
an insulated vessel containing 159 g of water at 22.8°C. Assuming
no loss of water and a heat capacity for the vessel of 10.0 J/°C,
what is the final temperature of the system (c of copper = 0.387
J/g·°C)?

7. Calorimetry A piece of metal has mass 100 grams and an
initial temperature of 100'C. lt is placed in an insulated
container of mass 200 grams which contains 500 grams of water at an
initial temperature of 17 .3"C. The container is made of the same
material as the metal sample. lf the final temperature is 22.7'C,
what is the specific heat capacity of this metal? How many calories
('1 cal = 4.186 J) are required to warm the...

A 15.3 gram piece of lead at 115.1 °C is placed in a calorimeter
containing water at 21.9 °C. If the temperature at equilibrium is
24.5 °C, what is the mass of the water?
Report your answer in grams to two (2) sig
figs.

A 39.9 gram piece of lead at 98.7 °C is placed in a calorimeter
containing water at 21.7 °C. If the temperature at equilibrium is
27.6°C, what is the mass of the water?

A 5.10 kg piece of solid copper metal at an initial temperature
T is placed with 2.00 kg of ice that is initially at -25.0 ∘C. The
ice is in an insulated container of negligible mass and no heat is
exchanged with the surroundings. After thermal equilibrium is
reached, there is 0.90 kg of ice and 1.10 kg of liquid water.
Part A
What was the initial temperature of the piece of copper?
Express your answer to three significant figures...

1.0 gram of copper and 1.0 gram of silver were both heated to
100 °C and then dropped into separate containers
of 10.0 grams of water at room temperature. When the systems come
to equilibrium, the container with the
silver will be at the higher temperature.
Question 1 options:
True
False

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 6 minutes ago

asked 10 minutes ago

asked 10 minutes ago

asked 12 minutes ago

asked 19 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 44 minutes ago

asked 54 minutes ago

asked 54 minutes ago

asked 55 minutes ago