Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have Χmethane = 0.915 and Χethane = 0.085.
a. What are the partial pressures of the two gases in a 15.00-L container of natural gas at 20.°C and 1.44 atm?
b. Assuming complete combustion of both gases in the natural gas sample, what is the total mass of water formed?
For part A is the total pressure given already, 1.44atm? So I would just multiplay the mole fraction times 1.44 giving partial pressures of (1.44*.915) = 1.32 atm for methane and (1.44*.085)=.1224 atm for ethane?
and for part B what might the equation be? CH4 + C2H6 + O2 = ?
Thanks for all your help.