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12 Dec 2019

Joan wishes to take a hot bath. She fills the tub with 320 Liters of water at temperature 52 degrees Celsius. Calculate the amount of energy required to raise the temperature of 320 Liters of water from 18 degrees Celsius to 52 degrees Celsius. It is useful to know that one liter of water has a mass of 1kg = 1000 g. Answer must be in joules. (4.184 joules per gram per degree Celsius)

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Jean Keeling
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13 Dec 2019

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Related questions

The heat energy associated with a change in temperature that does not involve a change in phase is given by

q=ms?T

where q is heat in joules, m is mass in grams, s is specific heat in joules per gram-degree Celsius, J/(g??C), and ?T is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by

q=m?H

where q is heat in joules, m is mass in grams, and ?H is the enthalpy in joules per gram.

Physical constants

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: ?Hfus=334 J/g

Enthalpy of vaporization: ?Hvap=2250 J/g

Part A

How much heat energy, in kilojoules, is required to convert 64.0 g of ice at ?18.0 ?C to water at 25.0 ?C ?

Express your answer numerically in kilojoules.

Submit

Part B

How long would it take for 1.50 mol of water at 100.0 ?C to be converted completely into steam if heat were added at a constant rate of 22.0 J/s ?

Express your answer numerically in minutes.

The heat energy associated with a change in temperature that does not involve a change in phase is given by

q=msΔT

where q is heat in joules, m is mass in grams, sis specific heat in joules per gram-degree Celsius, J/(g⋠∘C), and ΔT is the temperature change in degrees Celsius. The heat energy associated with a change in phase at constant temperature is given by

q=mΔH

where q is heat in joules, m is mass in grams, and ΔH is the enthalpy in joules per gram

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

Part A

How much heat energy, in kilojoules, is required to convert 75.0 g of ice at −18.0 ∘Cto water at 25.0 ∘C ?

Part B

How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 17.0 J/s ?

When 0.595 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.4 ∘C to 29.9 ∘C.

Part A

Find ΔErxn for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/∘C.

Part B

Learning Goal: To understand the concepts of heat capacity, specific heat, and molar heat capacity. Heat capacity, C, is the amount of energy required to raise the temperature of a substance by exactly 1 degree Celsius. The energy needed to warm an object increases as the mass of that object increases. We see this in our everyday life. For example, we know that it takes much more energy to heat a large tank of water than a small cup. Because of this dependence on mass, experimentally determined heat capacities are always reported in terms of the amount of the substance that is heated. One method is to report how much energy it takes to raise the temperature of one mole of a substance by exactly 1 degree Celsius. This value is the molar heat capacity, which has the symbol Cp.The molar heat capacity is given in the units J/(mol⋠∘C). A second method is to report how much energy it takes to raise the temperature of one gram of a substance by exactly 1 degree Celsius. This value is the specific heat, which has been given the symbol Cs. The units for specific heat are J/(g⋠∘C). The heat capacity of a substance is therefore related to the energy q needed to raise its temperature by an amount ΔT. That is, q=nCpΔT, where n denotes the number of moles of the substance, or q=mCsΔT, where m denotes the number of grams of the substance.

Part 1

It takes 55.0 J to raise the temperature of an 9.90 g piece of unknown metal from 13.0∘C to 24.8 ∘C. What is the specific heat for the metal?

Express your answer with the appropriate units.

Part 2

The molar heat capacity of silver is 25.35 J/mol⋠∘C. How much energy would it take to raise the temperature of 9.90 g of silver by 16.0 ∘C?

Express your answer with the appropriate units.

Part 3

What is the specific heat of silver? Express your answer with the appropriate units.

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