Specific Heat
Heat vs. Temperature
Fusion and Vaporization
Miscellaneous
Math, Math, Math
100
The equation that includes the heat added, mass, specific heat, and temperature
q=mc∆T
100
What is the form of energy that flows in and out of a system?
heat
100
The amount of heat required to convert a solid at its melting point into a liquid without an increase in temperature is what?
Heat of fusion
100
The amount of heat needed to raise an object's temperature 1 K
heat capacity
100
Solve for Gold's mass: c= 0.129 J/gºC q= 10 J ∆T= 10ºC
7.75 grams
200
This is the equation q=mc∆T... rearranged to solve for the mass of an object.
m=q/c∆T
200
What is the measure of kinetic energy called?
temperature
200
The amount of heat required to convert a unit mass of a liquid at its boiling point into vapor without an increase in temperature is what?
The heat of vaporization
200
The amount of heat required to raise the temperature of 1g of a substance by 1 K
specific heat
200
Solve for water's q value: c= 4.18 J/gºC m= 15 g ∆T= 3 ºC
188.1 Joules
300
The temperature of 300.0 g of water changed from 30.0 to 37.0ºC. How much energy was transferred into the water?
8800 J
300
In scientific work, temperatures are often expressed on what temperature scale?
Kelvins
300
List the steps needed to calculate the amount of heat required to completely convert 50 g of ice at -10 ºC to steam at 120 ºC.
1. The heating of ice 2. The melting of ice 3. The heating of water 4. The vaporization of water 5. The heating of the steam
300
A negative q value indicates what?
heat leaving the system
300
175 g of water at 10.0ºC was placed in a coffe cup calorimeter. 4.9 g of pure sulfuric acid at 10.0ºC was added to the calorimeter. The temperature rose to 14.9ºC. Assume the specific heat of the mixture to be 4.184 and all of the head produced is absorbed by the solution. How much heat was produced? Final answer in KJ
3.7 KJ
400
Which metal will lose heat the fastest? gold: .129 J/g°C chromium: .447 J/g°C copper: .385 J/g°C
Gold
400
What is the relationship between heat and temperature?
Temperature is a measure of the ability of a system to transfer heat energy to another system.
400
What is the heat in Joules required to melt 25 grams of ice? Molar mass of water: 18 g/mol Heat of fusion of water: 6.01 KJ/mol
8350 Joules
400
The amount of heat needed to raise the temperature of one mol of a substance 1 K
molar heat capacity
400
A negative 'Q' value stands for this...
What is HEAT LEAVING THE SYSTEM
500
What will be the temperature change if 1125J of energy is used to heat a block of iron weighing 0.5kg?(specific heat of iron is .450 J/g°C)
5°C
500
Which object contains the most heat, a boiling pot of water or a gigantic iceberg?
The gigantic iceberg
500
How much heat is released when 10 moles of steam, at 145°C is converted to ice at -20°C? molar heat of vaporization=40.7 KJ/mol molar heat of fusion=6.01 KJ/mol specific heat of steam=1.84 J/g-K Specific heat of ice=2.09 J/g-K
564.83 KJ
500
When 45.8 Joules are lost from water when gold is added to it, what is the amount of energy gained from the gold?
45.8 Joules
500
99 mL of 1.9 M H2O2 at 9°C is dropped into a calorimeter. The temperature in the calorimeter increases to 19.9°C. Assume the density of the solution to be 1.0 g/mL. Calculate the specific heat of H2O2 in KJ/mol.
24.0 kJ/mol
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