(a) A mixture containing 2.15 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L...

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Chemistry

(a) A mixture containing 2.15 g each ofCH₄(g), C₂H₄(g)and C₄H₁₀(g) is contained in a 1.50L flask at a temperature of 25Â°C.
Calculate the partial pressure of each of the gases in themixture.
P_CH₄ = ___ atm
P_C₂H₄ = ___ atm
P_C₄H₁₀ = _ atm
Calculate the total pressure of the mixture.
_ atm
(b) A mixture of gases contains 1.06 g of N₂, 2.22 gof H₂, and 1.22 g of NH₃. If the totalpressure of the mixture is 4.12 atm, what is the partial pressureof each component?
P_N₂ = ___ atm
P_H₂ = ___ atm
P_NH₃ = ___ atm

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4.0 Ratings (599 Votes)

a Given that a mixture containing 215 g each of CH4g C2H4g and C4H10g is contained in a 150 L flask at a temperature of 25C Ideal gas equation is PV nRT where n total moles sum of moles of individual components P total pressure of the mixure So first we have to find out the total moles of the mixture to get total pressure of the mixure Moles of CH4 mass of CH4 molar mass of CH4 215 g 16 gmol1 0134 moles Moles of C2H4 mass of C2H4 molar mass of C2H4 215 g 28 gmol1 0077 moles Moles of C4H10 mass of C4H10 molar mass of See Answer

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