As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm
1 Answers 1 viewsMolar mass of CH4 = 16.04 g/molMolar mass of argon = 39.9g/molFrom the given masses we can calculate number of moles followed by mole fraction of each gas.Number of moles...
1 Answers 1 viewsFirst, let's determine the total number of moles of both gases in the mixture at given conditions via Mendeleev-Clapeyron's law: PV=nRT; n=(PV)/(RT)= (101.3*10^3*5.04*10^-3)/(8.31*273)=0.225 mol. Then, let's write down to equations...
1 Answers 1 viewsAnswer: Let x = g C 3 H 4 and y = g C 2 H 6 equation 1 is x + y = 10.00 g C 3 H 4...
1 Answers 1 viewsAccording to Dalton's law of partial pressure:Ptotal = P1 + P2 + P3 ...where Ptotal - total pressure, Pn - partial pressureHere:Ptotal = PHe + PNe + PArAs a result,...
1 Answers 1 viewsThe partial pressure of each gas in a mixture is proportional to its mole fraction.n = m / MM (CO) = 28 g/molM (CO2) = 44 g/molM (CH4) = 16.04...
1 Answers 1 viewsP_gen=P(〖SO〗_2 )+P(N_2) P(〖SO〗_2 )= P_gen-P(N_2) 1 atm = 760 torr P(N_2 )=(760 torr×0.35 atm)/(1 atm)=266 torr P(〖SO〗_2 )= 520-266=254 (torr) Answer: 254 torr.
1 Answers 1 viewsp_i/p_total =x_i=n_i/n_total , where x_i- mole fraction. x_(〖CH〗_4 )= (0.145 atm)/((0.145+0.200) atm)×100%=42.0%; x_(O_2 )=(0.200 atm)/((0.145+0.200) atm)×100%=58.0%. Answer: x_(〖CH〗_4 )=42.0%; x_(O_2 )=58.0%.
1 Answers 1 views93.4 kPa
1 Answers 1 viewsMole fraction of N2- 0.208Mole fraction of Ne - 0.3Mole fraction of He - 0.458
1 Answers 1 views