The heat of combustion of methane is `-880 KJ mol^(-1)`. The quantity of heat liberated in the combustion of 3.2 g methane is

The heat of combustion of methane is, -880kJ mol^-1 . If 3.2 g of methane is burnt:

DeltaU of combustion of methane is -X kJ mol^-1 . The value of DeltaH is

DeltaU^@ of combustion of methane is -X kJ mol^(-1) . The value of DeltaH^@ is

DeltaU^(-) of combustion of methane is -x kJ mol^(-1) . The value of DeltaH^(-) is:

The heat of combustion of butane is 2880kJ" "mol^(-1) . What is the heat liberated by buring 1 kg of butane in excess of oxygen supply?

If the heat of combustion of pentane is 3507 kJ mol^(-1) then its calorific value will be ?

If the heat of combustion of pentane is 3507 kJ mol^(-1) then its calorific value will be ?