Part A: Calorimetry Tip for calorimetry problems: Always remember the 1" Law of Thermodynamics: energy cannot be created or destroyed, just converted from one form to another. In any calorimetry problem with multiple substances: if a substance releases heat, another substance is gaining it; the heat energy must come from somewhere and must go somewhere! q = mcAT will be the formula to use for all calorimetry problems, but keep in mind that negative q values mean a loss of heat, whereas positive q values mean a gain of heat. Note that the above formula is completely useless if there is no indication that a change in temperature ever occurred! What quantity of heat is required to raise the temperature of 55.5 g of gold from 20."C to 45°C? (specific heat of gold = 0.13 J/g"C) 1. If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (specific heat of silver = 0.24 J/g*C) 2. A 13.8-g piece of zinc at 98.9°C was dropped into 15.00 ml of water at 25.0°C. When the water and metal came to thermal equilibrium (i.e. there was no more net heat transfer between the water and metal), what was the temperature of the system? (specific heat of zinc = 0.388 J/g°C; specific heat of water = 4.184 J/g°C; density of water is approximately 1.000 g/mL) 3.
Part A: Calorimetry Tip for calorimetry problems: Always remember the 1" Law of Thermodynamics: energy cannot be created or destroyed, just converted from one form to another. In any calorimetry problem with multiple substances: if a substance releases heat, another substance is gaining it; the heat energy must come from somewhere and must go somewhere! q = mcAT will be the formula to use for all calorimetry problems, but keep in mind that negative q values mean a loss of heat, whereas positive q values mean a gain of heat. Note that the above formula is completely useless if there is no indication that a change in temperature ever occurred! What quantity of heat is required to raise the temperature of 55.5 g of gold from 20."C to 45°C? (specific heat of gold = 0.13 J/g"C) 1. If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (specific heat of silver = 0.24 J/g*C) 2. A 13.8-g piece of zinc at 98.9°C was dropped into 15.00 ml of water at 25.0°C. When the water and metal came to thermal equilibrium (i.e. there was no more net heat transfer between the water and metal), what was the temperature of the system? (specific heat of zinc = 0.388 J/g°C; specific heat of water = 4.184 J/g°C; density of water is approximately 1.000 g/mL) 3.
Chemistry
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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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Transcribed Image Text:Part A: Calorimetry
Tip for calorimetry problems:
Always remember the 1* Law of Thermodynamics: energy cannot be created or destroyed,
just converted from one form to another. In any calorimetry problem with multiple
substances: if a substance releases heat, another substance is gaining it; the heat energy
must come from somewhere and must go somewhere! q = mcAT will be the formula to use
for all calorimetry problems, but keep in mind that negative q values mean a loss of heat,
whereas positive q values mean a gain of heat. Note that the above formula is completely
useless if there is no indication that a change in temperature ever occurred!
What quantity of heat is required to raise the temperature of 55.5 g of gold from 20."c
to 45°C? (specific heat of gold = 0.13 J/g"C)
1.
2.
If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many
degrees will the temperature of the silver increase? (specific heat of silver = 0.24 J/g*C)
A 13.8-g piece of zinc at 98.9°C was dropped into 15.00 mL of water at 25.0°C. When
the water and metal came to thermal equilibrium (i.e. there was no more net heat
transfer between the water and metal), what was the temperature of the system?
(specific heat of zinc = 0.388 J/g°C; specific heat of water = 4.184 J/g°C; density of water
is approximately 1.000 g/mL)
3.
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