**Chemical Reaction Rate Law Problem**The rate law for the reaction \(A + B \rightarrow C\) was found to be:\[ \text{rate} = k[A][B] \]One experimental trial with the concentrations \([A] = 0.26 \, \text{M}\) and \([B] = 0.13 \, \text{M}\) had an initial rate of product formation of \(0.36 \, \text{M/s}\).**Question:**What is the value of the rate constant \(k\) for this reaction?**Answer:**Enter your answer as 0.0035 with no units. Use 2 significant digits.**Answer:** [ ]

Answered: Image /qna-images/answer/144597d7-f9b9-4291-a943-d3167a602e35.jpg

The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. Answer:

The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. 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...

See similar textbooks

Similar questions

Remember to use square brackets to show concentration. Do not include multiplication symbols in the rate equation. Do not place spaces in your answer. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO, (3) + CO(g) · NO (g) + CO,(g) Rate = X. He
-1 -1 At a certain temperature the rate of this reaction is second order in HI with a rate constant of 1.0M S 2HI (g) → H₂(g) + 1₂ (g) Suppose a vessel contains HI at a concentration of 1.33M. Calculate the concentration of HI in the vessel 7.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś ?
Consider this reaction: 2SO3 (g) →2SO₂ (g) +0₂ (8) At a certain temperature it obeys this rate law. rate = (2.99 M¹.5-¹) [SO] Suppose a vessel contains SO3 at a concentration of 0.160 M. Calculate the concentration of SO3 in the vessel 24.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0 x10 X G
A chemistry graduate student is studying the rate of this reaction: She fills a reaction vessel with and measures its concentration as the reaction proceeds: time (seconds) Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant . Round your answer to significant digits. Also be sure your answer has the correct unit symbol.
A chemistry graduate student is studying the rate of this reaction: NH,OH (aq) → NH, (aq) +H,0 (aq) 4 He fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds: time [NH,OH] (milliseconds) 0.0500M 10. 0.0178M 20. 0.0108M 30. 0.00778 M 40. 0.00607M
Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C1O₂(aq) + 2OH (aq)- ClO₂ (aq) + CIO, (aq) + H₂O(1) Under a certain set of conditions, the initial rate of disappearance of chlorine dioxide was determined to be 2.30 x 10 M/s. What is the initial rate of appearance of chlorite ion under those same conditions? 5.75 x 10-² M/s 4.60 x 10-¹ M/s A B 1.15 x 10-¹ M/s 2.30 x 10-¹ M/s E 9.20 x 10-¹ M/s
Use the table below to determine the rate law and rate constant for the reaction A + B → products. Justify your answer using words and/or calculations. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 1.00 1.00 0.250 2 2.00 2.00 2.000 3 3.00 1.00 0.750
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.
Question Use the initial rates method with the given data to determine the rate law for the hypothetical reaction shown below. A+B → C • Write the rate law in the form of rate = k[A]"[B]", specifying the value of the rate constant (k) and the reaction orders (m and n). • Include three significant figures in the rate constant. • Enter your answer in decimal form, do not use scientific notation. Trial [A] (mol/L) [B] (mol/L) 1 2 3 Provide your answer below: rate = 0.0300 0.0300 0.0600 0.0300 0.0600 0.0300 A[A] At (mol L-¹s-¹) 0.0004851 0.0004851 0.0019404
In a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 CH 3 NC(g) CH 3 CN(g) the concentration of CH 3 NC was followed as a function of time It was found that a graph of ln[CH 3 NC] versus time in seconds gave a straight line with a slope of - 4.17 * 10 ^ - 3 * s ^ - 1 and a y intercept of -4.05 Based on this plot , the reaction is order in CH 3 NC and the rate constant for the reaction is
A) If a reaction has the rate law v = k[A]1[B]0 then what is the power of M that appears in the units for k? A.1)If a reaction has the rate law v = k [A]0[B]3 then what is the power of M that appears in the units for k?
Please answer all parts.