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
To determine which statement is true, let's go through each option and analyze them one by one.
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.
The addition of a catalyst affects both the forward and reverse reactions equally by providing an alternative reaction pathway with a lower activation energy. Therefore, this statement is incorrect.
b. The value for the enthalpy of reaction would be decreased by the addition of a catalyst.
A catalyst does not affect the enthalpy of reaction. It only speeds up the rate at which the reactants are converted to products. Therefore, this statement is incorrect.
c. The reaction is endothermic.
To determine if the reaction is endothermic or exothermic, we need to compare the enthalpy of reaction to zero. In this case, the enthalpy of reaction is -20.0 kJ/mol, which is less than zero. This suggests that the reaction is exothermic, not endothermic. Therefore, this statement is incorrect.
d. The reverse reaction is slower than the forward reaction (smaller rate constant).
The activation energy for the forward reaction is given, but we do not have any information about the activation energy for the reverse reaction. Therefore, we cannot determine if the reverse reaction is slower or if the rate constant is smaller. This statement cannot be determined.
e. The reaction rate would be decreased by an increase in temperature.
For a one-step reaction, the rate of the reaction is typically directly proportional to the temperature. Therefore, if the temperature is increased, the reaction rate will also increase. This means that the reaction rate would not be decreased by an increase in temperature. Therefore, this statement is incorrect.
In conclusion, none of the given statements are true based on the information provided.