[" 1.00I 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 "1260cal/K" .The complete "],[" combustion of the methane to "CO_(2)&H_(2)O" caused a temperature rise in the calorimeter "0.667K" .What was "],[" the mole percent of "CH_(4)" in the original mixture? "],[Delta H_(comb)^(@)(CH_(4))=-215k" 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 of combustion of gaseous methan (CH_(4)) at constant volume is measured in a bomb calorimeter at 298 K and is found to be -885.4 kJ mol^(-1) .Find the value of enthalpy change.

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?

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?

The heat of combustion of gaseous methane (CH_(4)) at constant volume is measured in bomb calorimeter at 298K is found to be -885.4kjmol^(-1) . Find the value of enthalpy change at the same temperature.