A given hydrocarbon is burned in the presence of oxygen gas and is converted completely to water carbon dioxide the mole ratio of h2o to CO2 is 1.125:1.00 the hydrocarbon could be: a. C2H6
b. C3H4
c. CH4
d. C2H2
e. C4H9

omak

Explanation:

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in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)