Explain why the following statement is false: Increasing the temperature of a reaction increases the ratebecause it lowers the activation energy of the reaction.

Answered: Explain why the following sta because…

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...

See similar textbooks

Related questions

Question

Explain why the following statement is false: Increasing the temperature of a reaction increases the rate
because it lowers the activation energy of the reaction.

Expert Solution

Step 1

For a chemical reaction to occur, particles must collide. At a higher temperature particles move faster, increasing their kinetic energy and hence there are likely to be more collisions and hence rate of reaction increases.

For every rise of 10 °C in temperature usually doubles or triples the speed of a reaction between molecules.The minimum energy needed for a reaction to proceed, known as the activation energy, stays the same with increasing temperature.

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions