A gaseous alkane was exploded with oxygen. The volume of `O_(2)` for complete combustion to `CO_(2)` formed was in the ratio of `7:4`. The molecular formula of alkane is:

Answer

2

Explanation

`C_(n)H_(2n+2)+[n+(n+1)/(2)]O_(2)rarrnCO_(2)+(n+1)H_(2)O`
Given, `("vol.of"O_(2)"used")/("vol.of" CO_(2)"formed")=(7)/(4)`
`therefore (n+(n+1)//2)/(n)=(7)/(4) or n=2`