Draw a potential energy diagram with appropriately labelled axes to represent:
a) The exothermic combustion of octane ∆Ho
=-5.47MJ)
b) The endothermic formation of diborane (B2H6) from its elements ∆Ho
= +36kJ)
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To draw a potential energy diagram, we will use the reaction progress as the X-axis and the potential energy as the Y-axis. For each reaction, we will label the axes appropriately.
a) The exothermic combustion of octane (∆Ho = -5.47 MJ):
On the X-axis, we will label it as "Reaction Progress".
On the Y-axis, we will label it as "Potential Energy (kJ/mol)".
We will start with the reactants having a higher potential energy and move downwards towards the products.
At the beginning of the reaction, the reactants (octane and oxygen) have a higher potential energy. Label this point as "R" (for reactants).
As the reaction progresses, the potential energy decreases, indicating that energy is being released. Draw a downward sloping curve to show this.
At the end of the reaction, the products (carbon dioxide and water) have a lower potential energy. Label this point as "P" (for products).
Finally, label the energy change (∆Ho = -5.47 MJ) above the curve between the reactants and products.
The diagram should show a downward sloping curve from the reactant side to the product side, with the reactants at a higher potential energy and the products at a lower potential energy.
b) The endothermic formation of diborane (B2H6) from its elements (∆Ho = +36 kJ):
On the X-axis, we will label it as "Reaction Progress".
On the Y-axis, we will label it as "Potential Energy (kJ/mol)".
We will start with the elements (boron and hydrogen) having a higher potential energy and move downwards towards the product.
At the beginning of the reaction, the elements have a higher potential energy. Label this point as "E" (for elements).
As the reaction progresses, the potential energy increases, indicating that energy is being absorbed. Draw an upward sloping curve to show this.
At the end of the reaction, the product (diborane) has a higher potential energy than the elements. Label this point as "P" (for product).
Finally, label the energy change (∆Ho = +36 kJ) above the curve between the elements and product.
The diagram should show an upward sloping curve from the element side to the product side, with the elements at a higher potential energy and the product at a higher potential energy.
To draw a potential energy diagram representing the exothermic combustion of octane and the endothermic formation of diborane, you will need to understand the concept of potential energy and how it changes during a chemical reaction.
First, let's start with the exothermic combustion of octane. Exothermic reactions release energy, so the potential energy of the products will be lower than that of the reactants. Draw the vertical axis to represent potential energy, and label it accordingly. Place the reactants (octane) on the left side and label it with "C8H18". On the right side, place the products of combustion (carbon dioxide, water, etc.) and label it accordingly. Make sure to position the products lower on the potential energy axis to represent the release of energy.
For the endothermic formation of diborane, the process requires an input of energy, resulting in an increase in potential energy. Again, draw the vertical axis to represent potential energy and label it accordingly. Place the reactants (boron and hydrogen) on the left side and label them accordingly. On the right side, place the product (diborane) and label it accordingly. In this case, position the product higher on the potential energy axis to represent the increase in energy.
Remember to label the axes clearly and indicate the energy change (∆Ho) associated with each reaction.
Note: When drawing the potential energy curves, you may use smooth curves, line segments, or stair-step diagrams, depending on the level of detail you want to show.