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 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 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 viewsAnswer on Question #83513Container A holds 782 mL of ideal gas at 2.80 atm. Container B holds 174 mL of ideal gas at 4.40 atm. If the gases are allowed...
1 Answers 1 viewsLet the gas mixture be ideal.Then Dalton’s law: the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of each gas in...
1 Answers 1 viewsP is proportional to nPco2/PN2 = nco2/nN2Moles of gas is equal to the weight/molecular weight of gasPco2 is twice that of PN2Pco2 = 2PN2, weight of N2 = 9.05 gram2PN2/PN2...
1 Answers 1 viewsMass of nitrogen= 5.08 gNo.of mole of nitrogen= 5.08/28= .182Partial pressed of nitrogen let = PPV=nRTV=.182RT/PIn case of carbon dioxideMass of carbon dioxide=?Partial pressure of carbon dioxide= 2PPV=nRTn=PV/RTn=2P×.182RT/PRTn=.364 Mass of...
1 Answers 1 viewsp(CH4) = 0.55 atmp(C2H6) = 0.44 atmp(C3H8)= 0.51 atm
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