The reaction illustrated above is a combustive reaction where the endproducts are water and carbon dioxide as shown in the reaction productabove. In combustive reactions, there is always burning of substance whichreleases energy/heat to the surroundings of the system. We also see from theabove, that the change in heat (∆H) is given as ∆H= –1452.8 kJ/mol. Thenegative sign indicates a loss and more so, –1452.8 kJ/mol is less than zerowhich is an indication of energy/heat being released/loss from the systemhence an EXOTHERMIC reaction.b.What is the value of ∆H if the equation is multiplied throughout by 2? (2 points)Per the rules for thermochemical equations, when equation is multiplied throughby a factor, the change in heat/energy must also change by the same factor.Therefore, ∆H= 2 (–1452.8 kJ/mol) = –2905.6 kJ/molc.What is the value of ∆Hif the direction of the reaction is reversed so that the products become the reactants and vice versa? (2 points)If the direction of the reaction is reversed so that the products become the reactants and the reactants become the product, the value will be ∆H = +1452.8kJ/molThat is, magnitude of the value will remain the same but with a positive sign or a gain instead of a loss ( ∆H= 1452.8 kJ/mol) because the system would need same magnitude of energy/heat to yield the product except that in this case the system would be absorbing the energy from its surrounding thus undergoing an ENDOTHERMIC reaction which always yields a positive change or gain in energy/ heat change.