Answer:
-573.67
Explanation:
whenever energy is released in a chemical reaction, we would then expect the delta H of the reaction to be negative because the reaction is an exothermic reaction.
now we have that 2.81 moles of fuel when it combusts would releases 1612kJ of energy
thus, 1 mole will release 1612/2.81 = -573.67kJ of heat
Therefore the delta H of the reaction = -573.67 kJ/mol
The [tex]\Delta[/tex]H of the reaction for the combustion of the new fuel will be -573.66 kJ.
The enthalpy of reaction or [tex]\Delta[/tex]H of the reaction can be determined as the amount of heat required by the 1-mole substance formation.
The given potential fuel has 1,612 kJ of energy released for 2.81 moles of the fuel. The [tex]\Delta[/tex]H of the reaction has been the amount of energy released for the combustion of 1 mole of fuel.
According to the Unitary methods:
2.81 mol = 1,612 kJ
1 mol = [tex]\rm \dfrac{1612}{2.81}\;\times\;1[/tex]
1 mole = 573.66 kJ.
A negative sign has been imparted to the value of [tex]\Delta[/tex]H of the reaction, as there has been the release of the energy.
Thus, the [tex]\Delta[/tex]H of the reaction for the combustion of the new fuel will be -573.66 kJ.
For more information about the [tex]\Delta[/tex]H of the reaction, refer to the link:
https://brainly.com/question/3820658
