As you can see in the example, the volume in the gaseous state is higher than that in the liquid state at bolling. As a good approximation, we can ignore the initial volume occupied by the liquid. Now with 3.00 g of oxygen (molar mass = 32 g), assuming the gas is ideal, what is the change in internal energy as it vaporizes at its bolling point? AEt
As you can see in the example, the volume in the gaseous state is higher than that in the liquid state at bolling. As a good approximation, we can ignore the initial volume occupied by the liquid. Now with 3.00 g of oxygen (molar mass = 32 g), assuming the gas is ideal, what is the change in internal energy as it vaporizes at its bolling point? AEt
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If we Instead used 27.0 g of water, how much 100°C steam remains in thermal equilibrium?
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As you can see in the example, the volume in the gaseous state is higher than that in the liquid state at
bolling. As a good approximation, we can Ignore the initial volume occupled by the liquid. Now with 3.00
g of oxygen (molar mass = 32 g), assuming the gas is ideal, what is the change in internal energy as it
vaporizes at its bolling point?
AEint
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Transcribed Image Text:Physics
PLEASE BE CAREFULL WITH your
ANSWERS!!
MASTER IT
If we Instead used 27.0 g of water, how much 100°C steam remains in thermal equilibrium?
Additional Materials
leBook
As you can see in the example, the volume in the gaseous state is higher than that in the liquid state at
bolling. As a good approximation, we can Ignore the initial volume occupled by the liquid. Now with 3.00
g of oxygen (molar mass = 32 g), assuming the gas is ideal, what is the change in internal energy as it
vaporizes at its bolling point?
AEint
.......
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