## Chemistry and Chemical Reactivity (9th Edition)

Number of moles of butyl mercaptan: $0.095\ g\div90.184\ g/mol=1.05×10^{-3}\ mol$ From stoichiometry: Per molecule of combustion: $4\ CO_2, 5\ H_2O, 1\ SO_2$: 10 moles of gas formed $0.0105\ mol$ total $PV=nRT$ $P=0.0105\ mol×0.082057\ L.atm/mol.K×(25+273)\ K/5.25\ L$ $P=0.049\ atm$ Partial pressures, from Dalton's law: $P_{CO_2}=4/10×0.049\ atm=0.020\ atm$ $P_{H_2O}=5/10×0.049\ atm=0.024\ atm$ $P_{SO_2}=1/10×0.049\ atm=0.005\ atm$