Question

use the energy diagram below to fill in the blanks. the energy of the reactants is and the energy of the products is. we know that the reaction represented by this energy diagram is because the energy of the is greater than the energy of the reactants. this makes the heat of reaction have a sign with a numerical value of kj. the energy of the transition state/activated complex in kj is, making the activation energy of the reaction in kj. pe (kj) progress of the reaction a + b c + d 10 20 30 40 50 positive 10 20 40 50 exothermic endothermic products

Explanation:

Step1: Identify reactants energy

The energy of reactants $A + B$ is read from the y - axis at the start of the reaction. It is 10 kJ.

Step2: Identify products energy

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

Step3: Determine reaction type

Since the energy of the products (20 kJ) is greater than the energy of the reactants (10 kJ), the reaction is endothermic.

Step4: Determine heat of reaction sign and value

For an endothermic reaction, the heat of reaction ($\Delta H$) is positive. $\Delta H=E_{products}-E_{reactants}=20 - 10=10$ kJ.

Step5: Identify energy of transition state

The energy of the transition state/activated complex is the highest point on the energy - diagram, which is 50 kJ.

Step6: Calculate activation energy

Activation energy ($E_a$) is the difference between the energy of the transition state and the energy of the reactants. $E_a = 50-10 = 40$ kJ.

Answer:

The energy of the reactants is 10 kJ and the energy of the products is 20 kJ.
We know that the reaction represented by this energy diagram is endothermic because the energy of the products is greater than the energy of the reactants. This makes the heat of reaction have a positive sign with a numerical value of 10 kJ.
The energy of the transition state/activated complex in kJ is 50 kJ, making the activation energy of the reaction 40 kJ.