If O2(g) and H2(g) are in separate containers of equal pressure, volume and temperature, which one...
If O2(g) and H2(g) are in separate containers of equal pressure, volume and temperature, which one of these statements is true?
The amount of moles in the O2 container is greater than that in the H2 container.
There are more molecules in the H2 container than molecules in the O2 container.
If you increase the pressure in both containers, but keep temperature constant, the volume of both containers will increase
If you increase the pressure in both containers, but keep temperature constant, only the volume of the O2 container will increase
Both containers contain the same amount of molecules.
Homework Answers
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If O2(g) and H2(g) are in separate containers of equal pressure,
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8:54 LTE Question 6 of 23 Submit If two separate containers A and B have the same volume and temperature, but container A has more gaseous molecules than B, then container A will have: A) Higher pressure B) Lower presure C) A greater universal gas constant D) A smaller universal gas constant Tap here or pull up for additional resources
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