Question

A 200 g of copper, initially at 300o C, is dropped into a 350 g of water contained in a 355 g aluminum calorimeter; the water and the calorimeter are initially 15o C. If 25 g iron stirrer is used to bring the mixture into thermal equilibrium, what is the final temperature of the system? ( Assume that the stirrer is initially at 15o C.) Specific heat of copper and aluminum are 0.092 cal/g oC and 0.215 cal/g oC respectively. Also specific heat of water is 1.0 cal/g oC and that of iron is 0.106 cal/g oC. )

Answer #1

Solution in the uploaded image

A 100g block of copper initially at 100°C is dropped into 1000g
of water initially at 0℃. The specific heat of copper is 0.0923 ???
?℃ ,. What is the final temperature of the water and copper when
they reach thermal equilibrium?

A 25 g gold nugget with an initial temperature of 60 °C is
dropped into an insulated cup containing 100 ml of water initially
at a temperature of 5°C. What is the final temperature after
thermal equilibrium is established?
Table 3.4 Specific Heat Capacities of Some Common Substances
Substance Specific Heat Capacity (J/g °C) Lead 0.128 Gold 0.128
Silver 0.235 Copper 0.385 Iron 0.449 Aluminum 0.903 Ethanol 2.42
Water 4.184

If you were to dump 45.0 g of copper metal (specific heat =
0.092 cal/g°C) at 115°C into 75.0 g of water at 22.3°C, what
temperature will the final mixture be?

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 500-g aluminum container holds 300 g of water. The water and
aluminum are initially at 40∘C. A 200-g iron block at 0∘C is added
to the water. Assume the specific heat of iron is 450 J/kg⋅∘C, the
specific heat of water 4180 J/kg⋅∘C and the specific heat of
aluminum is 900 J/kg⋅∘C
.
1Determine the final equilibrium temperature.
2.Determine the change in thermal energy of the aluminum
3.Determine the change in thermal energy of the water. 4.
Determine...

A 59-kg iron block and a 20-kg copper block, both initially at
80°C, are dropped into a large lake at 15°C. Thermal equilibrium is
established after a while as a result of heat transfer between the
blocks and the lake water. Assuming the surroundings to be at 20°C,
determine the amount of work that could have been produced if the
entire process were executed in a reversible manner. The specific
heats of iron and copper are 0.45 kJ/kg·K and 0.386...

A 35.0-g cube of ice, initially at 0.0°C, is dropped into 180.0
g of water in an 70.0-g aluminum container, both initially at
35.0°C. What is the final equilibrium temperature? (Specific heat
for aluminum is 900 J/kg⋅°C, the specific heat of water is 4 186
J/kg⋅°C, and Lf = 3.33 × 105 J/kg.)
26.4 °C
17.6 °C
8.79 °C
35.1 °C
30.8 ° C

A 50 kg copper block initially at 350 oC is quenched in a
closed, rigid insulated tank containing 120 L of liquid water at 25
oC. Specific heat of copper, Cc = 385 J/(kgK), specific heat of
liquid water, Cw = 4180J/(kgK). (i) Calculate the entropy change
(kJ/K) of copper block. (ii) Determine the entropy change (kJ/K) of
liquid water.

In a copper vessel with a temperature of t1 = 350 C, m2 = 600 g
of ice
with a temperature of t1 = 10 C. After some time a
Mixture of m3 = 550 g ice and m4 = 50 g water. Find the mass of the
vessel m1.
In the solution, neglect the heat exchange between the vessel
and
environment.
The specific heat capacity of copper is cK = 0:39 kJ/(kg*K). The
specific
Heat capacity of the ice...

Part A
A copper pot of mass 2.5 kg contains 5.2 litres of water (i.e.
5.2 kg) at room temperature (200C). An iron block of
mass 9.4 kg is dropped into the water and when the system comes
into thermal equilibrium, a temperature of 380C is
measured. What is the initial temperature of the iron block? Give
your answer in oC to three significant figures.
Part B
Iron has a specific heat that is larger than that of copper. A...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 5 minutes ago

asked 5 minutes ago

asked 6 minutes ago

asked 8 minutes ago

asked 20 minutes ago

asked 28 minutes ago

asked 33 minutes ago

asked 36 minutes ago

asked 39 minutes ago

asked 47 minutes ago

asked 49 minutes ago