Answer:
In the reaction you provided:
A + B -> C + 36 kJ/mol
The enthalpy change (ΔH) for the forward reaction is given as 36 kJ/mol. This means that 36 kJ of energy are released for every mole of reactants A and B that are converted into products C. In this case, since energy is being released (exothermic reaction), the products have lower energy compared to the reactants.
The activation energy (Ea) for the forward reaction is given as 73 kJ/mol. Activation energy is the minimum energy required for the reactants (A and B) to overcome the energy barrier and initiate the reaction. In this case, it takes 73 kJ/mol of energy input to get the reaction started.
To summarize:
ΔH (enthalpy change) = -36 kJ/mol (negative because it's an exothermic reaction, meaning energy is released)
Ea (activation energy) = 73 kJ/mol (the energy needed to initiate the reaction)
The negative sign in ΔH indicates that the reaction is exothermic, meaning it releases energy as it proceeds from reactants to products. The positive activation energy (Ea) indicates that there is an energy barrier that must be overcome for the reaction to occur, but once that barrier is crossed, the reaction proceeds with the release of 36 kJ/mol of energy.
Step-by-step explanation: