Question

fill the the blank with the appropriate answer based on the energy diagram below: the energy of the reactants is (in kj) and the energy of the products is (in kj). this means that the heat of reaction or △h is (in kj). because of the heat in reaction that means that this reaction is the energy of the transition state/or activated complex (in kj) is this means the activation energy (in kj) for this reaction shown below is pe (kj) a + b c + d progress of the reaction endothermic exothermic -20 20 40 60 100

Explanation:

Step1: Identify reactant energy

The energy of reactants A + B is read from the y - axis at the start of the reaction. It is 40 kJ.

Step2: Identify product energy

The energy of products C + D is read from the y - axis at the end of the reaction. It is 20 kJ.

Step3: Calculate heat of reaction

The heat of reaction $\Delta H$ is given by $\Delta H=H_{products}-H_{reactants}$. So, $\Delta H = 20 - 40=- 20$ kJ.

Step4: Determine reaction type

Since $\Delta H<0$, the reaction is exothermic.

Step5: Identify transition - state energy

The energy of the transition state is the maximum energy point on the curve, which is 100 kJ.

Step6: Calculate activation energy

The activation energy $E_a$ is the difference between the energy of the transition state and the energy of the reactants. So, $E_a=100 - 40 = 60$ kJ.

Answer:

The energy of the reactants is 40 kJ.
The energy of the products is 20 kJ.
The heat of reaction or $\Delta H$ is - 20 kJ.
This reaction is Exothermic.
The energy of the transition state/ or activated complex is 100 kJ.
The activation energy for this reaction is 60 kJ.