Heat of a reaction is defined as the amount of heat absorbed or evolved at a given temperature when the reactants have combined to form the products is represented by balanced chemical equation. If the heat is denoted by q then the numerical value of q depends on the manner in which
the reaction is performed for two methods of conducting chemical reactions in calorimeters.
The heat of combustion of maltose at a constant volume in the above question if water vapour is not condensed will be:
The correct option is B -1343 kcal/mol
q=ΔE+PΔV or q=ΔE+ΔngRT
where ΔE= the heat of combustion in calorimeteric bomb.
On putting values we get