In a reaction of a potential new fuel, it is found that when 2.81 moles of the fuel combusts, 1,612 kJ of energy is released. What is the delta Hrxn for the combustion of the fuel in units of kJ/mol. (If it is negative, include the negative sign

The H of the reaction for the combustion of the new fuel will be -573.66 kJ.

The enthalpy of reaction or 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 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 =

1 mole = 573.66 kJ.

A negative sign has been imparted to the value of  H of the reaction, as there has been the release of the energy.

Thus, the H of the reaction for the combustion of the new fuel will be -573.66 kJ.

For more information about the H of the reaction, refer to the link:

link

-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

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