Equal Volumes Ideal Gases: Same Temp, Pressure- A or C?

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Equal volumes of different ideal gases at the same temperature and pressure contain the same number of molecules, which corresponds to option C, "the same amount of gas." The discussion clarifies that since the gases are not specified as 24 dm³, options B and D can be eliminated. The gas equation confirms that the number of molecules is equal, but the distinction between atoms in different gases, such as helium and hydrogen, complicates the understanding of option A. Ultimately, the focus is on the equality of gas amounts rather than the number of atoms. The conclusion emphasizes that the correct interpretation aligns with the concept of equal amounts of gas in terms of moles.
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"Equal volumes of different ideal gases at the same temperature and pressure must contain:"

A. The same number of atoms
B. one mole of each gas
C. The same amount of gas
D. 6.022 x 10^23 particles of each gas


Since it is not 24dm^3 of each gas, I can rule out B and D.

After rearranging the gas equation:

NRT/P = NRT/P

N = N

The molar ratios are equal, but i don't know which of A or C is correct since i don't see the difference.
 
Physics news on Phys.org
helium molecule contain one atom, hydrogen molecule contain two atom...
and the N in your equation represent number of molecule...
so the answer is...
 
Thank you!
 
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