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 of the following statements is true?

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

Both containers contain 6.022 x10^23 molecules of gas.

Both containers have the same number of molecules.

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

Both containers have the same number of molecules
As they have the same values for pressure, volume and temperature so have the same amount of moles thus the same number of molecules as (number of molecules=(moles*Avagadro’s constant) )

They would only both contain 6.022*10^23 molecules if they both were at STP as at STP you would only have 1 mole of each gas.

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tutorareej tutorareej · Answer 2 · 2021-11-19T17:31:03+01:00

The hydrogen and oxygen gases present at the same temperature and pressure and have equal volume are consisted of the same number of molecules. Thus, statement c is correct.

The number of molecules present in a volume of gas been has been given by the Avogadro number. The Avogadro number has the number of molecules present in a mole of gas.

The container containing the hydrogen and oxygen gas is present at the same temperature and pressure. According to the ideal gas equation, if two gases are present at the same temperature and volume and have the same volume, the number of mole of the two gases has been equal.

Since both hydrogen and oxygen are consisted of the same moles of gases, according to the Avogadro concept, the number of molecules of gases has been equal.

Thus, the hydrogen and oxygen gases present at the same temperature and pressure and have equal volume are consisted of the same number of molecules. Thus, statement c is correct.

For more information about the molecules of gases, refer to the link:

https://brainly.com/question/2696683