### Understanding Activation Energy in Chemical ReactionsChemical reactions often require an initial input of energy to occur, known as activation energy. The activation energy is the minimum energy required for reactants to undergo a chemical transformation. This concept is crucial in determining the rate and likelihood of chemical reactions.#### Example Scenario:**Reaction A** has a high activation energy, whereas **Reaction B** has a low activation energy. **Question**: Which of the statements about Reaction A and Reaction B are true?1. [ ] Reaction B is likely to occur at a faster rate than Reaction A.2. [ ] Reaction A is likely to occur at a faster rate than Reaction B.3. [ ] Reaction B is more likely to occur at all than Reaction A.4. [ ] Reaction A is more likely to occur at all than Reaction B.Understanding the statements:- **Statement 1**: This suggests that **Reaction B** will happen faster because it has a lower activation energy.- **Statement 2**: This suggests that **Reaction A** will happen faster, which is unlikely due to its higher activation energy.- **Statement 3**: This suggests that **Reaction B** is more probable to happen because it requires less energy to initiate.- **Statement 4**: This suggests that **Reaction A** is more probable, which contradicts its high activation energy.**Explanation**: Generally, reactions with lower activation energy proceed faster and are more likely to occur because they need less energy to get started. Therefore, in this case, statements 1 and 3 are likely to be true.---This question helps students assess the relationship between the activation energy of reactions and their likelihood and rate of occurrence. Understanding these principles is fundamental in fields such as chemistry, biology, and environmental science.

the activation energy of a chemical reaction is closely related to its rate specifically the higher…

Reaction A has a high activation energy, whereas reacton B has a low activation energy. Which of the statements about reaction A and reaction B are true? Reaction B is likely to occur at a faster rate than reaction A. Reaction A is likely to occur at a faster rate than reaction B. Reaction B is more likely to occur at all than reaction A. Reaction A is more likely to occur at all than reaction B.

Reaction A has a high activation energy, whereas reacton B has a low activation energy. Which of the statements about reaction A and reaction B are true? Reaction B is likely to occur at a faster rate than reaction A. Reaction A is likely to occur at a faster rate than reaction B. Reaction B is more likely to occur at all than reaction A. Reaction A is more likely to occur at all than reaction B.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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