Question

If 0.16 mol of O₂ gas has a volume of 7.20 L at a certain temperature and pressure, what volume does 0.47 moles of O ₂ have under the same conditions?

Answer 1

To solve this problem, we can use the concept of the molar volume of a gas at constant temperature and pressure. The molar volume represents the volume occupied by one mole of a gas under those conditions.

Given: Initial moles of O₂ gas (n1) = 0.16 mol Initial volume (V1) = 7.20 L Final moles of O₂ gas (n2) = 0.47 mol

We can set up a proportion using the molar volumes:

V1 / n1 = V2 / n2

Substituting the given values:

7.20 L / 0.16 mol = V2 / 0.47 mol

Now, we can solve for V2 by rearranging the equation:

V2 = (7.20 L * 0.47 mol) / 0.16 mol

V2 ≈ 21.15 L

Therefore, 0.47 moles of O₂ gas would have a volume of approximately 21.15 L under the same temperature and pressure conditions.