At and pressure, of a hydrocarbon required of for complete combustion and of is formed. The formula of the hydrocarbon is

Question

At  and  pressure,  of a hydrocarbon required  of  for complete combustion and  of  is formed. The formula of the hydrocarbon is

Canvas Classes · Accepted Answer

Strategy:
 For gaseous hydrocarbons, use the general combustion equation: . At constant temperature and pressure, volume ratios are identical to mole ratios.

Step 1: Find carbon count (x) from } \ce{CO2} 	ext{ volume
 of Hydrocarbon yields  of .
Since  mole of  gives  moles of :

Step 2: Find hydrogen count (y) from } \ce{O2} 	ext{ volume
 of Hydrocarbon consumes  of .

Step 3: Assemble the formula
The hydrocarbon is .

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