An ideal gaseous mixture of ethane `(C_(2)H_(6))` and ethene `(C_(2)H_(4))` occupies `28` litre at `1atm` `0^(@)C`. The mixture reacts completely with `128 gm O_(2)` to produce `CO_(2)` and `H_(2)O`. Mole of fraction at `C_(2)H_(6)` in the mixtture is-

A mixture of ethane (C_(2)H_(6)) and ethene (C_(2)H_(4)) occupies 40 L at 1.00 atm and at 400 K . The mixture reacts completely with 130 g of O_(2) to produce CO_(2) and H_(2)O . Assuming ideal gas behaviour, calculate the mole fractions of C_(2)H_(4) and C_(2)H_(6) in the mixture.

A gaseous mixture contains 4.0g of H_(2) and 56.0g of N_(2) . The mole fraction of H_(2) in the mixture is

A gaseous mixture contain CH_(4) and C_(2)H_(6) in equimolecular proportion. The weight of 2.24 litres of this mixture at NTP is

A mixture of C_(2)H_(2) and C_(3)H_(8) occupied a certain volume at 80mm Hg. The mixture was completely burnt to CO_(2) and H_(2)O (I). When the pressure of CO_(2) was found to be 230mm Hg at the same temperature and volume, the fraction of C_(2)H_(2) in mixture is .