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Question

Flask A contains H2 gas and B contains CH4 gas have equal mass and volume at 300 K and 600 K respectively. Which flask will have a greater number of molecules?
(Assuming ideal behaviour for both the gases.)

A
A
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B
B
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C
Both A and B are equal
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D
None
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Solution

The correct option is A A
Let nA be the number of molecules of H2 and nB be the number of molecules of CH4.

We know that,
nA=m2;nB=m16

where m is the mass of the gas of two flasks A and B.

nAnB=m2/m16=8

Now, the number of molecules in these flasks are given as :

NA=m2×N,NB=m16×N
where N is Avogadro's constant.

NANB=8

NA>NB

Hence, option (A) is correct.

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