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One goal is to understand _____ for calculations
Heating and cooling curve
Another goal is to understand the __ of molar enthalpy
definition
As you move from the solid to the liquid to the gas form, what must happen?
heat must be absorbed from the environment
As you move from the gas to the liquid to the solid form, what must happen?
Heat must be released to the environment
What is Deposition?
when a substance goes directly from gas to solid
What is sublimation?
when a substance goes directly from solid to gas
What is the molar enthalpy of fusion?
amount of energy needed to melt 1 mole of ice
What is the molar enthalpy of fusion equation?
Q = nΔHfusion
What is n =?
moles of ice
What is ΔH?
enthalpy change (J/mol)
Enthalpy =
heat divided by the number of moles
What equation should be used for 3 different phases in the Heating Curve?
Q = mcΔT
In Q = mCΔT, what is m?
mass
In Q = mcΔT, what is c?
specific heat
Does the specific heat of ice, water, and water vapor all defer from eachother?
yes
What equation should be used for melting on the heating curve?
Q = nΔHfusion
What equation should be used for vaporization on the heating curve?
Q = nΔHvaporization
You must use the specific heat of ice in the equation until the temp reaches:
0 degrees C (freezing temp of water)
You must use the specific heat of water in the equation until the temp reaches:
100 degrees C (boiling temp of water)
You must use the specific heat of water vapor in the equation if the temp:
is more than 100 degrees C
When we add ice to hot water in the lab, what will we measure and what will we use?
Coffee Cup Calorimeter & the heat exchange between the water and ice
How do you add the substance to the calorimeter?
push the side of the inverted cup to create an opening
Fill 600ml beaker with:
deionized water
Warm DI water to?
70-75 degrees C
What should you do after adding the ice?
weigh the paper towel
Work __ after ice is added
quickly
Specific heat of ice?
2.09 J/g°C
Specific heat of water?
4.18 J/g°C
Specific heat of water vapor/steam?
1.86 J/g°C