Is the amount of energy it will absorb per unit of physical properties. erty can be measured quite accurately and is called specific heat (Cp). Specific heat is the amount of energy, measured in joules, needed to raise the temperature of one gram of the substance one Celsius degree. Often applied to metallic elements, specific heat can be used as a basis for comparing energy absorption and transfer. To measure specific heat in the laboratory, a calorimeter of some kind must be used. A calorimeter is a well-insulated container used in measuring energy changes. The calorimeter is insulated to reduce the loss or gain of energy to or from the surroundings. Energy always flows from an object at a higher temperature to an object at a lower temperature. The heat gained by the cooler substance equals the heat lost by the warmer substance, if we assume no loss of heat to the surrounding environment. HEAT LOST = HEAT GAINED In this experiment you will determine the specific heat of a metal sample. The metal sample will be heated to a high temperature then placed into a calorimeter containing a known quantity of water at a lower temperature. Having measured the mass of the water in the calorimeter, the temperature change of the water (AT), and knowing the specific heat of water (4.184J/g °C), the heat gained by the water (lost by the metal) can be calculated as follows. qwater metal (m* AT Cp) water (m* AT Cp) metal * * (mATCP) water (mAT) metal CPmetal= Watch the video on canvas and complete the pre-lab assignment before starting the experiment. Feel free to use a separate sheet of paper. Pre-lab Questions: (Answers are given to numerical questions to aid you.) 1. What physical properties, other than specific heat, could you use to help you identify the sample used in this experiment?
Is the amount of energy it will absorb per unit of physical properties. erty can be measured quite accurately and is called specific heat (Cp). Specific heat is the amount of energy, measured in joules, needed to raise the temperature of one gram of the substance one Celsius degree. Often applied to metallic elements, specific heat can be used as a basis for comparing energy absorption and transfer. To measure specific heat in the laboratory, a calorimeter of some kind must be used. A calorimeter is a well-insulated container used in measuring energy changes. The calorimeter is insulated to reduce the loss or gain of energy to or from the surroundings. Energy always flows from an object at a higher temperature to an object at a lower temperature. The heat gained by the cooler substance equals the heat lost by the warmer substance, if we assume no loss of heat to the surrounding environment. HEAT LOST = HEAT GAINED In this experiment you will determine the specific heat of a metal sample. The metal sample will be heated to a high temperature then placed into a calorimeter containing a known quantity of water at a lower temperature. Having measured the mass of the water in the calorimeter, the temperature change of the water (AT), and knowing the specific heat of water (4.184J/g °C), the heat gained by the water (lost by the metal) can be calculated as follows. qwater metal (m* AT Cp) water (m* AT Cp) metal * * (mATCP) water (mAT) metal CPmetal= Watch the video on canvas and complete the pre-lab assignment before starting the experiment. Feel free to use a separate sheet of paper. Pre-lab Questions: (Answers are given to numerical questions to aid you.) 1. What physical properties, other than specific heat, could you use to help you identify the sample used in this experiment?
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Transcribed Image Text:Is the amount of energy it will absorb per unit of
physical properties.
erty can be measured quite accurately and is called specific heat (Cp).
Specific heat is the amount of energy, measured in joules, needed to raise the
temperature of one gram of the substance one Celsius degree. Often applied to
metallic elements, specific heat can be used as a basis for comparing energy
absorption and transfer.
To measure specific heat in the laboratory, a calorimeter of some kind must be used. A
calorimeter is a well-insulated container used in measuring energy changes. The
calorimeter is insulated to reduce the loss or gain of energy to or from the surroundings.
Energy always flows from an object at a higher temperature to an object at a lower
temperature. The heat gained by the cooler substance equals the heat lost by the
warmer substance, if we assume no loss of heat to the surrounding environment.
HEAT LOST = HEAT GAINED
In this experiment you will determine the specific heat of a metal sample. The metal
sample will be heated to a high temperature then placed into a calorimeter
containing a known quantity of water at a lower temperature. Having measured the
mass of the water in the calorimeter, the temperature change of the water (AT), and
knowing the specific heat of water (4.184J/g °C), the heat gained by the water (lost
by the metal) can be calculated as follows.
qwater qmetal..
(m* AT Cp) water (m* AT Cp) metal
*
*
CPmetal=
(mAT Cp) water
(mAT) metal
Watch the video on canvas and complete the pre-lab assignment before starting the
experiment. Feel free to use a separate sheet of paper.
Pre-lab Questions:
(Answers are given to numerical questions to aid you.)
1. What physical properties, other than specific heat, could you use to help you identify
the sample used in this experiment?
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