Answer
See the answer below.
Work Step by Step
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:
$P_{CO_2}=4/10×0.049\ atm=0.020\ atm$
$P_{H_2O}=5/10×0.049\ atm=0.024\ atm$
$P_{SO_2}=1/10×0.049\ atm=0.005\ atm$
