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A given reaction has an energy difference between reactants and products (\(\Delta H\)) of -23.7 kJ/mol and a forward activation energy (AE) of 27.9 kJ/mol. Which of the following are possible values of \(\Delta H\) and AE for the forward reaction in the presence of a catalyst? Select all that apply.

A. \(\Delta H = -12.1 \, \text{kJ/mol}\) and \(\text{AE} = 10.3 \, \text{kJ/mol}\)
B. \(\Delta H = -43.9 \, \text{kJ/mol}\) and \(\text{AE} = 50.4 \, \text{kJ/mol}\)
C. \(\Delta H = -23.7 \, \text{kJ/mol}\) and \(\text{AE} = 10.3 \, \text{kJ/mol}\)
D. \(\Delta H = -9.27 \, \text{kJ/mol}\) and \(\text{AE} = 50.4 \, \text{kJ/mol}\)
E. \(\Delta H = -23.7 \, \text{kJ/mol}\) and \(\text{AE} = 99.1 \, \text{kJ/mol}\)
F. \(\Delta H = -23.7 \, \text{kJ/mol}\) and \(\text{AE} = 21.2 \, \text{kJ/mol}\)

Answer :

The correct options are:

- H = -12.1 kJ/mol and AE = 10.3 kJ/mol

- H = -23.7 kJ/mol and AE = 10.3 kJ/mol

- H = -9.27 kJ/mol and AE = 50.4 kJ/mol

- H = -23.7 kJ/mol and AE = 21.2 kJ/mol

A catalyst does not change the energy difference between reactants and products (H) or the overall energy profile of the reaction. It only provides an alternative pathway with a lower activation energy (AE). Therefore, the value of H should remain the same in the presence of a catalyst, which is -23.7 kJ/mol. However, the AE can be lowered by the catalyst, but it cannot be lower than the absolute value of H because the activation energy is the energy barrier that must be overcome to reach the transition state, and the reaction must have a higher energy transition state than the products.

Let's analyze each option:

1. H = -12.1 kJ/mol and AE = 10.3 kJ/mol

- This option is possible because the catalyst can lower the activation energy. The H value is less exothermic than the original reaction, which is not typical for a catalyst, but it is not impossible for a reaction with multiple steps where the catalyst only affects some of the steps.

2. H = -43.9 kJ/mol and AE = 50.4 kJ/mol

- This option is not possible because the H value is more exothermic than the original reaction, which a catalyst cannot do. A catalyst does not change the thermodynamics of the reaction, only the kinetics.

3. H = -23.7 kJ/mol and AE = 10.3 kJ/mol

- This option is possible because the H remains the same, and the catalyst lowers the AE, which is a typical effect of a catalyst.

4. H = -9.27 kJ/mol and AE = 50.4 kJ/mol

- This option is possible because, again, the catalyst can lower the activation energy. The H value is less exothermic than the original reaction, which could happen in a multi-step reaction as mentioned earlier.

5. H = -23.7 kJ/mol and AE = 99.1 kJ/mol

- This option is not possible because the AE is higher than the original reaction's AE, which means the catalyst is not effective in lowering the energy barrier.

6. H = -23.7 kJ/mol and AE = 21.2 kJ/mol

- This option is possible because the H remains the same, and the catalyst lowers the AE to a value that is still higher than the absolute value of H, which is consistent with the role of a catalyst.

In summary, a catalyst can lower the activation energy but does not change the enthalpy change of the reaction (H). The options where H is different from the original reaction's H are not possible unless the catalyst is altering the reaction pathway in a way that changes the overall thermodynamics, which is not typical for a catalyst. The options where AE is lowered compared to the original reaction's AE are possible and consistent with the role of a catalyst.

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Rewritten by : Barada

The correct answer is option c ΔH = -23.7 kJ/mol and AE = 10.3 kJ/mol

What is catalyst?

A catalyst is a substance that increases the rate of a chemical reaction by lowering the activation energy required for the reaction to occur, without undergoing any permanent chemical change itself. Catalysts work by providing an alternative pathway for the reaction that has a lower activation energy, allowing more reactant molecules to participate in the reaction and increasing the rate of product formation. Catalysts are widely used in industrial processes to increase the efficiency of chemical reactions and reduce the amount of energy required to produce a given amount of product. Some common examples of catalysts include enzymes in biological systems, transition metals such as platinum and palladium used in catalytic converters in cars, and acid or base catalysts used in the production of many chemicals.

Due to this, The activation energy (AE) is the minimum energy required to initiate a chemical reaction, and a catalyst can lower the activation energy required for a reaction to occur. However, a catalyst does not change the overall energy difference between the reactants and products (ΔH) of the reaction. Therefore, the only possible value for ΔH in the presence of a catalyst is still -23.7 kJ/mol.

Of the given answer choices, only ΔH = -23.7 kJ/mol and AE = 10.3 kJ/mol is a possible combination . The activation energy can be lowered to any value less than the original value of 27.9 kJ/mol, but it cannot be increased. Therefore, only the lower value of AE = 10.3 kJ/mol is a possible value in the presence of a catalyst.

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