What is the volume, in L, of 2.50 moles of oxygen gas measured at 25.0oC and a pressure of 104.5 kPa?

58.53 L

Explanation:

Ideal gas equation is

PV = nRT

P - the pressure of the gas = 104.5  KPa

V- the volume occupied by the gas

n  - the number of moles of gas =2.50

R - the universal gas constant, usually given as  0.0821 atm.L/(mol K)

T - the absolute temperature of the gas.= 298K

Now substituting vales we get

V = 58.53 L

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.