Complete combustion of a 0.0150 mol sample of a hydrocarbon,CxHy, gives 3.024 L of CO2 at STP and 1.891 g of H2O.
(a) What is the molecular formula of the hydrocarbon?
(b) What is the empirical formula of the hydrocarbon?
A 0.500-L bulb containing Ne at 685 torr is connected by a valveto a 2.50-L bulb containing CO2 at 375 torr. The valve between thetwo bulbs is opened and the two gases mix. The initial gaspressures as known to three significant figures.
(a) What is the partial pressure (torr) of Ne?
(b) What is the partial pressure (torr) of CO2?
(c) What is the total pressure?
(d) What is the mole fraction of Ne?
