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.

Question

Aydan Carney

Chemistry

9 June, 08:46

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.

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Zoe Bowen · Answer 1

False, False, False

Explanation:

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. 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.