Asample of oxygen gas (o2) has a volume of 7.51 l at a temperature of 19°c and a pressure of 1.38 atm. calculate the moles of o2 molecules present in this gas sample. a. 0.217 mol b. 0.866 mol c. 6.65 mol d. 0.433 mol =n

The moles of O₂ which are present in the sample are 0.433. (option D)

Explanation:

We should apply the Ideal Gases Law, to solve this:

P . V = n. R. T

1.38 atm . 7.51L = n . 0.082 . 292K

(1.38 atm . 7.51L) / (0.082 . 292K) = n

0.433 moles = n

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey