Question

Which of the following is not true for an exothermic reaction?

A. the products have a higher enthalpy than reactants
B. the temperature of the surroundings rise
C. the enthalpy change for the reaction is negative heat flows from the rxn system to the surroundings

Answer 1

The false statement regarding an exothermic reaction is: A. the products have a higher enthalpy than reactants

Step-by-step explanation:

An exothermic reaction is a type of chemical reaction that involves the release of energy from the system to the surroundings. Thus increasing the temperature of the surroundings.

In this reaction, the enthalpy or energy of the reactants is greater than the enthalpy or energy of the products. (
`\Delta H_(f) (Products) < \Delta H_(f) (reactants)`)

As the enthalpy change of a reaction:
`\Delta H_(r) = \sum \Delta H_(f) (Products) - \sum \Delta H_(f) (reactants)`

Therefore, the enthalpy change for an exothermic reaction is negative (
`\Delta H_(r) < 0`)