Q5 - Half-lifeHomework • Unansweredlodine atoms combine to form molecular iodine in the gas phase. This second order reaction has a rate constant of 7.0 x 1091/(M*s). Calculate the time required for the iodine concentration to decrease from 0.60 M (t=0) to 0.30 M.Note: this specific time is known as the half-life of the reaction.|(g) + I(g) → I2(g)->|2{8)Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer.a2.4 x 10-10 sb9.9 x 10-11 s4.3 x 10-11 s

Given Initial Concentration = 0.6 M Final Concentration = 0.3 M Rate constant = 7 × 109 M-1s-1

Q5 - Half-life Homework • Unanswered lodine atoms combine to form molecular iodine in the gas phase. This second order reaction has a rate constant of 7.0 x 109 1/(M*s). Calculate the time required for the iodine concentration to decrease from 0.60O M (t=0) to 0.30 M. Note: this specific time is known as the half-life of the reaction. |(g) + I(g) → I2(e) + |(g) |2(8) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 2.4 x 10-10 s b 9.9 x 10-11 s 4.3 x 10-11 s

Q5 - Half-life Homework • Unanswered lodine atoms combine to form molecular iodine in the gas phase. This second order reaction has a rate constant of 7.0 x 109 1/(M*s). Calculate the time required for the iodine concentration to decrease from 0.60O M (t=0) to 0.30 M. Note: this specific time is known as the half-life of the reaction. |(g) + I(g) → I2(e) + |(g) |2(8) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 2.4 x 10-10 s b 9.9 x 10-11 s 4.3 x 10-11 s

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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Part A A first-order reaction (AB) has a half-life of 25 minutes. If the initial concentration of A is 0.900 M, what is the concentration of B after 50 minutes? (Do not use a calculator to solve this problem.) Express your answer with the appropriate units. [B] = Submit ovide Feedback ■ μA Value Request Answer @ C Units ? Review | Constants I Periodic Table P Pearson MacBook Pro Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | Nex
A chemical engineer is studying the rate of this reaction. H_CO, (aq) + H,O (aq)+CO,(aq) He fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds. Here's a graph of his data: [H₂CO₂] (M) 08- 04- 02+ 0+ 02 0.6 1 (s) What is the half life of the reaction? 0.8 Use this graph to answer the following questions: Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in H₂CO3. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H₂CO3 in the engineer's reaction vessel after 2.00 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H₂CO3. Round your answer to 2 significant digits. = k = 0 0₁ [H.CO,] = M Ox 0.0 X 4
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Remaining Time: 2 hours, 22 minutes, 53 seconds. Question Completion Status: Below is the initial rate data from a few experiments on the reaction: A+B> Products. [A]; (M) Experiment # 11 12 3 The reaction is first order in A. The rate constant is thus: O 5.656 Ms-1 O 2.828 M-1-1 O 11.31 s-1 O 1.414 M-25-1 1.00 2.00 2.00 QUESTION 7 Consider the following reaction: O Equal to the rate of reaction. O Three times the rate of reaction O Twice the rate of reaction One third of the rate of reaction [B]; (M) 2 03(g) -> 3 O2(g) What is the rate of consumption of O3 compared to the rate of reaction? O Half of the rate of reaction. 1.00 .00 2.00 Click Save and Submit to save and submit. Click Save All Answers to save all answers. Rate; (M s-1) 1.414 2.828 11.31 İy S
Use the attached data to plot a graph "ln a as a function of time" for both 20ºC and 30ºC. Use the equation: y=-mx +b where y is ln a, m is k, x is time. Does this poor confirm a first order reaction? If so, how do you know?
1 4 7 +/- lodine-123 is a radioactive isotope used to study thyroid gland functions. It decays in a first-order process with a half life of 786 min. You receive a sample for some of your experiments, but you have to work fast before it is all gone. Calculate the NUMBER OF HOURS it will take for 95% of your sample to decay. 2 LO Question 16 of 20 5 8 hrs 3 6 9 0 Submit Tap here or pull up for additional resources X C x 100
What is half-life [in hours] for a first-order reaction which has a rate constant of 7.6*10-5 s-1? There is an error in the book's version: the rate constant should have a negative exponent.