Question

Suppose that Daniel has a 3.00 L bottle that contains a mixture of O2 , N2 , and CO2 under a total pressure of 5.30 atm. He knows that the mixture contains 0.310 mol N2 and that the partial pressure of CO2 is 0.350 atm. If the temperature is 273 K, what is the partial pressure of O2 ?

Answer 1

pressure. According to dalton's law of Pertial P= P + P + bgt.... where p = Total Pressure B = Pestial Pressure of gars't B of gas '2' Now the Pertial Pressure b = h, RT v h₂ RT - MRT we have Volume Cus= 3.00L Temperature (T) = 273K R = 0.082 L-atm not kn numbers of molesct N₂ = 0.310 mol : (0.310 m01) X (9.0822matmmodali)) X (2736) 3.00L atm = 2.313 Pestial Total Pressure at coa = Peop= 0.350 atm Pressure (P) - s.30atm. : P= Prat Pont Por or s.30atm = 2.313 atm + 0.350 atm & Pee Po = 2.637 atm. & Pestial Pressure of O₂ = Pour 2.637 abr.