Indicate whether each statement is true or false. If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. Exothermic reactions are faster than endothermic reactions. If you double the temperature for a reaction, you cut the activation energy in half.

If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. FALSE. The relation between the rate constant (k) and the activation energy (Ea) is given by the Arrhenius equation, that is, k depends on the Ea, but not on the enthalpy (ΔH).

Exothermic reactions are faster than endothermic reactions. FALSE. Whether a reaction is exothermic or endothermic is defined by the sign of the enthalpy. However, as stated previously, the rate constant (and the rate reaction) do not depend on the enthalpy of the reaction.

If you double the temperature for a reaction, you cut the activation energy in half. FALSE. The activation energy does not depend on the temperature.

andromache andromache · Answer 2 · 2022-04-12T12:43:38+02:00

When the rate constant should be determined so we cannot calculate the enthalpy change.

The Exothermic reactions should not be faster.

Indication of the statement:

here the relationship that lies between the rate constant and the activation energy that should be provided by the Arrhenius equation should be based on the Ea.

In the case when the reaction should be considered as the exothermic so it represent the sign of the enthalpy.

Also, the activation energy does not based upon the temperature.

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