why will no one answer this question?

For a one step reaction, the activation energy for the forward reaction is 40.0 kJ/mol and the enthalpy of reaction is -20.0 kJ /mol. Which statement below is true?

a. The activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction by addition of a catalyst.

b. The value for the enthalpy of reaction would be decreased by addition of a catalyst.

c. The reaction is endothermic.

d. The reverse reaction is slower than the forward reaction (smaller rate constant).

e. The reaction rate would be decreased by an increase in temperature.

i have no idea how to do this, i hate ap chem

To answer this question, you need to understand the concepts of activation energy, enthalpy of reaction, and the effect of a catalyst on a reaction. Here's a step-by-step explanation of how to approach and answer this question:

1. Recall that activation energy is the energy required to start a chemical reaction. It determines the rate at which a reaction occurs.

2. In the given information, the activation energy for the forward reaction is 40.0 kJ/mol. This means that it takes 40.0 kJ/mol of energy to initiate the forward reaction.

3. The enthalpy of reaction is a measure of the heat energy exchanged during a chemical reaction. In this case, the enthalpy of reaction is -20.0 kJ/mol. The negative sign indicates that the reaction is exothermic, meaning it releases heat energy.

Now let's analyze the statements and determine which one is true:

a. The activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction by the addition of a catalyst.

To evaluate this statement, you need to know how a catalyst affects the activation energy of a reaction. A catalyst lowers the activation energy by providing an alternative reaction pathway with a lower energy barrier. This reduction in activation energy affects both the forward and reverse reactions equally.

Since the statement suggests that the activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction, it is not true. Therefore, option a is false.

b. The value for the enthalpy of reaction would be decreased by the addition of a catalyst.

A catalyst does not affect the enthalpy change of a reaction. It only speeds up the rate of reaction by reducing the activation energy. Therefore, option b is false.

c. The reaction is endothermic.

The enthalpy of reaction is given as -20.0 kJ/mol, indicating that the reaction is exothermic, not endothermic. Option c is false.

d. The reverse reaction is slower than the forward reaction (smaller rate constant).

The rate constant for a reaction depends on the activation energy and temperature. The information provided does not indicate any difference in the activation energies or temperatures for the forward and reverse reactions. Therefore, option d does not hold true.

e. The reaction rate would be decreased by an increase in temperature.

According to the Arrhenius equation, increasing the temperature increases the rate of reaction. This is because higher temperatures provide more energy to overcome the activation energy barrier. Therefore, option e is false.

In summary, none of the given statements are true.