For the following questions, use the reaction SO3(g) SO2(g) + O2(g), with ÄH = 98.4 kJ/mol and ÄS = 0.09564 kJ/(mol·K). (8 points)
i. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction. (2 points)
ii. Is the reaction endothermic or exothermic? Explain your answer. (2 points)
iii. What is the Gibbs free energy of the reaction at 300 K? (2 points)
iv. Is the reaction spontaneous or nonspontaneous at 300 K? Explain your answer.
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i. To draw a potential energy diagram of the reaction, first, understand the concept. A potential energy diagram shows the change in potential energy throughout a chemical reaction.
In this case, we have the reaction:
SO3(g) → SO2(g) + O2(g)
The vertical axis of the potential energy diagram represents the potential energy of the system, and the horizontal axis represents the progress of the reaction from reactants to products.
Start by drawing a curve that represents the initial potential energy of the reactant, SO3(g). Label this point as "Reactants." Then, draw a line or curve that shows the change in potential energy as the reaction progresses to the products, SO2(g) and O2(g). Label this point as "Products."
As for labeling the enthalpy of the reaction, you need to consider whether the reaction is exothermic or endothermic.
ii. To determine if the reaction is endothermic or exothermic, consider the enthalpy change (ΔH) of the reaction. In this case, ΔH is given as 98.4 kJ/mol.
An exothermic reaction releases heat (energy) to the surroundings, resulting in a negative ΔH value. On the other hand, an endothermic reaction absorbs heat (energy) from the surroundings, resulting in a positive ΔH value.
Since ΔH is positive (98.4 kJ/mol), it indicates an endothermic reaction. Therefore, label the enthalpy of the reaction as a positive value on the potential energy diagram.
iii. To calculate the Gibbs free energy (ΔG) of the reaction at 300 K, use the equation:
ΔG = ΔH - TΔS
Where ΔH is the enthalpy change and ΔS is the entropy change. T is the temperature in Kelvin.
Given: ΔH = 98.4 kJ/mol, ΔS = 0.09564 kJ/(mol·K), and T = 300 K.
Substitute the values into the equation:
ΔG = 98.4 kJ/mol - (300 K)(0.09564 kJ/(mol·K))
Calculate the result to find the ΔG value.
iv. To determine if the reaction is spontaneous or nonspontaneous at 300 K, analyze the sign of ΔG.
If ΔG is negative, the reaction is spontaneous. If ΔG is positive, the reaction is nonspontaneous.
Calculate the value of ΔG using the equation mentioned in part iii. If the calculated ΔG value is negative, label the reaction as spontaneous at 300 K. If the calculated ΔG value is positive, label the reaction as nonspontaneous at 300 K.
By following these steps, you should be able to answer all the given questions and explain how to get the answers.