Question

Specific Heat The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature. Note the difference between the terms |
Use the following values: specific heat of water = 4.18 J/(g⋅∘C) specific heat of steel = 0.452 J/(g⋅∘C) Express your answer to three significant figures and include the appropriate units.
The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar heat capacity of water. Express your answer to three significant figures and include the appropriate units.
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Answer #1

A)

Density of water = 1.00 g/mL

Density = mass/volume

1.00 = mass/120

mass = 120 g

m_{1}C_{p}_{1}T_{1} =
m_{2}C_{p2}T_{2}

where 1 represents water and 2 represents steel rod

120 4.18
(22.0 - 21.20) = m_{2} 0.452
(21.20 - 2.00)

m_{2} = 46.2 g

B)

Mol mass of water = 18 g/mol

18 g/mol x 4.18 J/g.°C = 75.24 J/mol.^{o}C (or K).

Specific Heat
The heat capacity of an object indicates how much energy that
object can absorb for a given increase in that object's
temperature. In a system in which two objects of different
temperatures come into contact with one another, the warmer object
will cool and the cooler object will warm up until the system is at
a single equilibrium temperature.
Note the difference between the terms molar heat
capacity, which has units of J/(mol⋅∘C), andspecific
heat, which has units...

Part A) A volume of 90.0 mL of H2O is initially at room
temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in
the water. If the final temperature of the system is 21.50 ∘C ,
what is the mass of the steel bar? Use the following values:
specific heat of water = 4.18 J/(g⋅∘C) specific heat of steel =
0.452 J/(g⋅∘C) Express your answer to three significant figures and
include the appropriate units.
Part B)
The...

Part A
A volume of 80.0 mL of H2O is initially at room temperature
(22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water.
If the final temperature of the system is 21.30 ∘C ,
what is the mass of the steel bar?
Use the following values:
specific heat of water = 4.18 J/(g⋅∘C)
specific heat of steel = 0.452 J/(g⋅∘C)
Express your answer to three significant figures and include the
appropriate units.
The specific heat of...

Part A:
A volume of 95.0 mL of H2O is initially at room temperature
(22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water.
If the final temperature of the system is 21.00 ∘C ,
what is the mass of the steel bar?
Use the following values:
specific heat of water = 4.18 J/(g⋅∘C)
specific heat of steel = 0.452 J/(g⋅∘C)
Part B:
The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar
heat capacity of...

A volume of 110. mL of H2O is initially at room temperature
(22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water.
If the final temperature of the system is 21.20 ∘C , what is the
mass of the steel bar? Use the following values: specific heat of
water = 4.18 J/(g⋅∘C) specific heat of steel = 0.452 J/(g⋅∘C)

A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C)
is placed in a boiling water bath until the temperature of the
metal is 100.0*C. The metal is quickly transferred to 119.0g of
water at 25.0*C in a calorimeter (specific heat capacity of water =
4.18 J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is
placed in a boiling water bath until the temperature of the metal
is 100.0*C. The metal is quickly transferred to 119.0g of water at
25.0*C in a calorimeter (specific heat capacity of water = 4.18
J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

How much heat energy, in kilojoules, is required to convert 46.0
g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to
three significant figures and include the appropriate units.
The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250
J/g

How much heat energy, in kilojoules, is required to convert 79.0
g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to
three significant figures and include the appropriate units.
The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250
J/g

The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar
heat capacity of water.

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