A proposed mechanism for a reaction is:

(i) A + B2 = AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol
(ii) AB2 + C2 = ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol
(iii) ABC + B2 = AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8
kJ/mol

a) Which is the rate determining step? Explain why.

(ii) It requires the greatest increase in energy, and thus, is the slowest.

b) What is the overall equation for this reaction?

A + 2B2 + C2 = AB2 +2BC deltaH= 0.4 kj/mol

c) Name a reaction intermediate.

ABC

d) Draw a completely labeled energy diagram to scale for the overall reaction. Clearly show deltaHr
and Ea.

?????

Please help!! Please check my work and help with d)

To draw the energy diagram for the overall reaction, we can combine the individual steps and their respective energies.

The overall reaction can be obtained by adding the equations (i), (ii) and (iii) together:

A + B2 + C2 = AB2 + BC (overall equation)

Now, let's draw the energy diagram:

Energy
|
_______ | (iii)
|
_______ | (ii)
|
_______ | (i)
|
_______ |
|
Reactants Products
(A + B2 + C2) (AB2 + BC)

On the energy diagram, the y-axis represents the energy and the x-axis represents the progress of the reaction. Starting from the left, we have the reactants (A + B2 + C2) at a certain energy level. As the reaction progresses, it goes through each step, labeled (i), (ii), and (iii), which correspond to the individual reactions.

The Ea values represent the energy barriers to overcome for each step. The reaction will proceed fastest when the energy barrier is the lowest. In this case, step (iii) has the lowest Ea value of 10 kJ/mol, so it is the rate-determining step.

The deltaH values represent the enthalpy change for each step. However, since we do not know the enthalpy change for the individual steps, we cannot accurately represent deltaH on the energy diagram without that information.

Note: The deltaH value provided (0.4 kJ/mol) seems to be for the overall reaction, not for any specific step.

To determine the rate determining step (RDS), you need to look at the step with the highest activation energy (Ea). In this case, step (ii) has the highest Ea of 30 kJ/mol. This means it requires the most energy to proceed, making it the slowest step. Therefore, step (ii) is the rate determining step.

For the overall equation, you need to combine the individual steps, canceling out species that appear on both sides:

(i) A + B2 = AB2
(ii) AB2 + C2 = ABC + BC
(iii) ABC + B2 = AB2 + BC

By combining these steps, you get the overall equation:

A + 2B2 + C2 = AB2 + 2BC

The delta H for the overall reaction will be the sum of the enthalpy changes for each step:

delta H = deltaH1 + deltaH2 + deltaH3
= (3 kJ/mol) + (5.2 kJ/mol) + (-7.8 kJ/mol)
= 0.4 kJ/mol

So the overall enthalpy change for the reaction is 0.4 kJ/mol.

To draw a completely labeled energy diagram for the overall reaction, you would need to plot the energy on the y-axis and the reaction progress on the x-axis. Since I can't draw here, I'll explain the key points on the diagram:

1. Start with the reactants A, B2, and C2 on the left side at a certain energy level.
2. Draw a line representing the energy change for step (i), going up by 12 kJ/mol.
3. Draw another line representing the energy change for step (ii), going up by 30 kJ/mol above the ending level of step (i).
4. Draw a line representing the energy change for step (iii), going down by 10 kJ/mol below the ending level of step (ii).
5. Finally, draw a line connecting the ending level of step (iii) to the right side representing the products AB2 and BC at a certain energy level.

Make sure to label the energy changes (Ea values) for each step and the overall enthalpy change (delta H).