Question

A 20.95 g piece of iron and a 25.20 g piece of gold at 100.0 celsius were dropped into 570.0 ml of water at 27.95 celsius. The molar heat capacities of iron and gold are 25.19 J/(mol*celsius) and 25.41 J/(mol*celsius), respectively. What is the final temperature of the water and pieces of metal?

Answer #1

A 155g piece of iron (Cp = 25.09J/mol. degree Celsius) was
heated to a temperature of 52 degrees Celsius and then placed in
contact with a 270g piece of copper at 10 degrees Celsius (Cp =
25.46 J/mol. degrees Celsius). What was the final temperature of
the two pieces of metal degrees Celsius?

If a piece of Cd with a mass = 37.6 g and initial temperature of
100.0 o C is dropped in 25.0 mL
of water at 23 o C, what is the final temperature of the system?
specific heat of Cd = 0.232
J/g o C; specific heat of water = 4.184 J/g o C.

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.

Exactly 17.7 mL of water at 35.0 °C are added to a hot iron
skillet. All of the water is converted into steam at 100.0°C. The
mass of the pan is 1.20 kg and the molar heat capacity of iron is
25.19 J/(mol·°C). What is the temperature change of the
skillet?

A piece of iron weighing 20.0 g at a temperature of
95.0ºC was placed in 100.0 g of
Water at 25.0ºC. Assuming that no
heat is lost to the surroundings, what is the resulting temperature
of the iron and water?

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

A hot lump of 45.0 g of iron at an initial temperature of 68.2
degrees celsius is placed in 50.0 mL of H2O initially at 25.0
degrees celsius and allowed to reach thermal equillibrium. What is
the final temperature of the iron and water given that the specific
heat of iron is 0.449 J/(G x degrees celsius)? Assume no heat is
lost to surroundings.

1. What is the final temperature of a solution initially at 22.0
celsius if 2.45 g of a solid is dropped into 34.5 g of the solution
resulting in the reaction between the two that absorbs 1350 J of
heat?
2. If a 31.25g piece of an unknown metal at 25 Celsius was added
to 25.0 g of water at 100.0Celsius and the two equilibrated at 95.2
Celsius , what is the specific heat capacity of the metal?
3. In...

Problem 5.54
A 100.0-g bar of gold is heated from 25 ∘C to 50 ∘C during which
it absorbs 322 J of heat. Assume the volume of the gold bar remains
constant.
Part A
Based on the data, calculate the specific heat of
Au(s).
Express your answer to two significant figures and include the
appropriate units.
Cs =
0.13 J⋅(g⋅∘C)−1
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Part B
Suppose that the same amount of heat is added...

1. A 74.2-g piece of metal is heated to 89.55 degrees C and
dropped into 52.0 g of water at 23.22 degrees C in a calorimeter
with the heat capacity of 41.0 J/C . The
final temperature of the system is 27.60 degrees C.
a) Assuming that the metal does not react with water and
Cs(H2O) = 4.18 J/g*C , calculate
the specific heat capacity of the metal in
J/g*C
b) Most metals have the same molar heat capacity of...

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