Question

Analyze the graph determine which statement is true? A.) The excess energy produced is absorbed by the surrounding area B.) The catalyze reaction requires more activation energy C.) The catalyze reaction requires less energy D.) Both reactions occur at the same way of time

Answer 1

The correct statement based on the graph is that the catalyzed reaction requires less energy. Catalysts lower the activation energy required for a reaction without changing whether a reaction is exothermic or endothermic.

Step-by-step explanation:

Analyzing the graph regarding a chemical reaction with and without a catalyst, it should be clear that certain statements are either true or not based on the information provided. For a catalyzed reaction, we can discuss activation energy, the energy necessary for the reaction to begin.

Catalysts function by providing an alternative pathway for the reaction with a lower activation energy than the uncatalyzed reaction. This means that the catalyzed reaction requires less energy, not more. If the analysis shows that the activation energy is lower when the catalyst is present, the correct statement is that the catalyzed reaction requires less energy.

Exothermic and endothermic reactions are terms that relate to whether a reaction releases or absorbs energy, respectively. A catalyst doesn't affect whether a reaction is exothermic or endothermic; it simply provides a lower energy route for the reaction. Hence, we cannot determine if the reaction is absorbing or releasing energy to or from the surroundings solely based on the activation energies.