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You have two containers at 25°C and 1 atm. One has 22.4 L of hydrogen gas, and the other has 22.4 L of oxygen gas.

Which statement is true?


The hydrogen gas container has more molecules than the oxygen gas container.


The oxygen gas container has more molecules than the hydrogen gas container.


Both containers have the same number of molecules.


Both containers contain 6.022×1023 molecules of gas.

Sagot :

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Both containers have the same number of molecules= 5.62 x 10²³

Further explanation

Given

22.4 L of hydrogen gas

22.4 L of oxygen gas

25°C and 1 atm.

Required

true statement

Solution

Conditions at T 25 ° C and P 1 atm are stated by RTP (Room Temperature and Pressure). Vm in this condition = 24 liters / mol

and from Avogadro's Law :

At the same temperature and pressure, the ratio of gas volume will be equal to the ratio of gas moles  

So two gas have the same molecules

1 mol = 6.02 x 10²³ molecules

24 L = 1 mol, so for 22.4 L :

[tex]\tt \dfrac{22.4~L}{24~L}\times 6.02\times 10^{23}~molecules=5.62\times 10^{23}~molecules[/tex]

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