Consider two 5 L chambers. In one, there are 5.00 g of [tex]O_2[/tex], and in the other, there are 5.00 g of He. Which chamber has the higher pressure at room temperature?

The chamber containing helium would have a higher pressure at room temperature. This is because, according to the ideal gas law, the pressure of a gas is dependent on the number of its molecules (or moles) and not its mass. Given the molar masses of helium and oxygen, there would be more moles of helium in the chamber.

Explanation:

The question asks which of the two 5l chambers, one containing 5.00g of oxygen (O2) and the other containing 5.00g of helium (He), would have a higher pressure at room temperature. This is a Chemistry problem focused on gas laws. According to the ideal gas law, the pressure of a gas depends on the number of molecules (or moles) present in the chamber, not the mass. Taking into consideration the molar masses of oxygen and helium - approximately 32g/mol and 4g/mol respectively - there would be more moles of helium in the chamber than oxygen. So, the helium-filled chamber would be under higher pressure at room temperature.

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