Determine the number of moles of each gas present in a mixture of CH4 and C2H6 i

Question

Determine the number of moles of each gas present in a mixture of CH4 and C2H6 in a 2.00 L vessel at 25C and 1.40 atm given the partial pressure of CH4 is 0.37atm.

What is the numer of moles of CH4? ____ mol

What is the number of moles of C2H6? _____ mol

Determine the partial pressure and number of moles of each gas in a 14.25 L vessel at 30.0C containing a mixture of xenon and neon gases only. The total pressure in the vessel is 5.10 atm, and the mole fraction of xenon is 0.731.

What is the partial pressure of xenon? _____atm

What is the partial pressure of neon? ____ atm

What is the number of moles of xenon? ____ mol

What is the number of moles of neon? ____ mol

Explanation / Answer

Total moles = PV/RT = 1.4*2/(0.0821*(25+273.15) =0.114388

Moles of CH4+ moles of C2H6= 0.114388

Partial pressure of C2H6= 1.4-0.37= 1.03 atm

Partial pressure of CH4/ Total pressure = moles of CH4/ total moles

0.37/1.4= moles of CH4/0.114388

Moles of CH4= 0.0302 moles

Moles of C2H6= total moles- moles of CH4= 0.114388-0.0302=0.08188

b)

Total moles= PV/RT= 5.1*14.25/ (0.0821*(30+273.15))=2.92 moles

Moles of Xenon =mole fraction * total moles = 0.731*2.92=2.134

Moles of neon= 2.92-2.134=0.786

Partial pressure = mole fraction * total pressure

Partial pressures : Xeon : 0.731*5.1=3.73 atm   and partial pressure of neon= total pressure-partial pressure of Xe=5.1-3.73=1.37 atm

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