**Problem Statement:**A first-order reaction has a half-life of 21.9 seconds. How long does it take for the concentration of the reactant in the reaction to decrease to one-fourth of its initial value?**Instructions:**Express the time to three significant figures and include the appropriate units.**Input Fields:**- There is an input box labeled “t =” with two fields: - **Value**: Enter the numerical value. - **Units**: Specify the units.**Buttons:**- **Submit**: To submit the answer.- **Previous Answers**: To view past attempts.- **Request Answer**: To ask for the solution.**Toolbar Options:**- Contains various formatting tools, including: - Structuring input - Undo/redo actions - Accessing the keyboard - Help section**Note:** Ensure accuracy and precision in your calculation.

For the first order reaction : k = 0.693/t0.5 = 0.693/21.9 s = 0.0316 s^-1. Hence, the rate…

A first-order reaction has a half-life of 21.9 s . How long does it take for the concentration of the reactant in the reaction to fall to one-fourth of its initial value? Express the time to three significant figures and include the appropriate units. HA ? t = Value Units Submit Previous Answers Request Answer

A first-order reaction has a half-life of 21.9 s . How long does it take for the concentration of the reactant in the reaction to fall to one-fourth of its initial value? Express the time to three significant figures and include the appropriate units. HA ? t = Value Units Submit Previous Answers Request Answer

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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