1.00 `l` sample of a mixture of `CH_(4) (g)` & `O_(2)(g)` measured at `25^(@)C` & `740` torr was allowed to react at constant pressure in a calorimeter which together with its contents had a heat capacity of 1260 Cal/K. The Complete combustion of methane to `CO_(2)` & `H_(2)O` caused a temperature rise, in the Calorimeter, of 0.667 K. What was the mole percent of `CH_(4)` in the original mixture ?
`DeltaH_("comb")^(@) (CH_(4))=-215" k Cal mol"^(-1)`.

1.0 litre sample of a mixture of CH_(4) and O_(2) measured at 25^(@)C and 740 torr, was allowed to react at constant pressure in a calorimeter, together with its contents had a heat capacity of 1260 cal K^(-1) . The complete combustion of CH_(4) to CO_(2) and water caused a temperature rise in calorimeter of 0.667K . Calculate mole % of CH_(4) in the original mixture. Heat of combustion of CH_(4) is -210.8 kcal.

1.0 litre sample of a mixture of CH_(4) and O_(2) measured at 25^(@)C and 740 tor r , was allowed to react at constant pressure in a calorimeter, together with its contents had a heat capacity of 1260 cal K^(-1) . The complete combustion of CH_(4) to CO_(2) and water caused a temperature rise in calorimeter of 0.667K . Calculate mole % of CH_(4) in the original mixture. Heat of combustion of CH_(4) is -210.8 kcal.

One litre sample of a mixture of CH_(4) and O_(2) measured at 32^(@)C and 760 torr, was allowed to react at constant pressure in a calorimeter which together with its content has a heat capacity of 1260 cal/degree. The complete combustion of CH_(4) to CO_(2) and water caused a temperature rise in calorimeter of 0.667K . calculate mole % of CH_(4) in original mixture. [Given: Heat of combustion of CH_(4) is -210.8 Kcal//mol . Total heat capacity of the calorimeter = 2108 cal K ]

One litre sample of a mixture of CH_(4) and O_(2) measured at 32^(@)C and 760 torr, was allowed to react at constant pressure in a calorimeter. The complete combustion of CH_(4) to CO_(2) and water caused a temperature rise in calorimeter of 1K . calculate mole % of CH_(4) in original mixture. [Given: Heat of combustion of CH_(4) is -210.8 Kcal//mol . Total heat capacity of the calorimeter = 2108 cal K ]

The heat librerated on complete combustion of 1 mole of CH_(4) gas to CO_(2)(g) and H_(2)O(l) is 890 kJ. Calculate the heat evolved by 2.4 L of CH_(4) on complete combustion.

A container of 1 L capacity contains a mixture of 4 g of O_(2) and 2 g H_(2) at 0 ^(@)C . What will be the total pressure of the mixture ?

A sample of CH_(4) of 0.08 g was subjected to combustion at 27^(@)C in a bomb calorimater. The temperature of the calorimeter system was found to be raised by 0.25^(@)C . IF heat capacity of calorimeter is 18K J, Delta H for combustion of CH_(4) at 27^(@)C is

A mixture of CH_(4) and C_(2)H_(2) occupied a certain volume at a total pressure equal to 63 torr. The same gas mixture was burnt to CO_(2) and H_(2)O(l).CO_(2)(g) alone was collected in the same volume and at the same temperature, the pressure was found to be 99 torr. What was the mole fraction of CH_(4) in the original gas mixture?