When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 4.53 g of NH4CIO4(s) are dissolved in 111.60 g of water, the temperature of the solution drops from 24.02 to 21.06 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.81 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4CIO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AH dissolution kJ/mol
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 4.53 g of NH4CIO4(s) are dissolved in 111.60 g of water, the temperature of the solution drops from 24.02 to 21.06 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.81 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of NH4CIO4(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AH dissolution kJ/mol
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![When a solid dissolves in water, heat may be evolved or absorbed.
The heat of dissolution (dissolving) can be determined using a
coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 4.53
g of NH4CIO4(s) are dissolved in 111.60 g of water, the
temperature of the solution drops from 24.02 to 21.06 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was determined in a separate experiment to
be 1.81 J/°C.
Based on the student's observation, calculate the enthalpy of
dissolution of NH4CIO4(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat
of water.
AH dissolution =
kJ/mol
Thermometer
Cardboard or
Styrofoam lid
Nested
Styrofoam cups
Reaction
occurs in
solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6f999b7-6deb-4015-91d6-5f59e418959d%2F3e9e7c63-324a-4024-bd02-a55a409dea89%2Fr7cqg7e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:When a solid dissolves in water, heat may be evolved or absorbed.
The heat of dissolution (dissolving) can be determined using a
coffee cup calorimeter.
In the laboratory a general chemistry student finds that when 4.53
g of NH4CIO4(s) are dissolved in 111.60 g of water, the
temperature of the solution drops from 24.02 to 21.06 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was determined in a separate experiment to
be 1.81 J/°C.
Based on the student's observation, calculate the enthalpy of
dissolution of NH4CIO4(s) in kJ/mol.
Assume the specific heat of the solution is equal to the specific heat
of water.
AH dissolution =
kJ/mol
Thermometer
Cardboard or
Styrofoam lid
Nested
Styrofoam cups
Reaction
occurs in
solution.
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