8 need help please

Question

A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.93 bar at 298 K . She knows that the mixture contains 0.221 mol N2 and that the partial pressure of CO2 is 0.343 bar . Calculate the partial pressure of O2 .

Answer 1

To start, 1 bar=0.9869 atm. According to Dalton's Law of Partial Pressure, P_Total= sum of the partial pressures. wew know the partial pressure of the CO₂, and we can calculate the partial pressure of the N₂. If PV=nRT, and we know the moles of N₂ (0.221), the P=nRT/V, or P=0.(221 mol)(0.08206L-atm/mole-K)(298K), P=1.81 atm=1.84 bar. P_Total=4.93 bar=P_N2 + P_CO2 + P_O2=1.84 + 0.343 +P_O2. P_O2=2.75 bar.