Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.259 0.549 0.0232 Trial 2 0.518 0.549 0.0928 Trial 3 0.259 1.10 0.0232 Trial 4 0.783 0.210 0.212 Rate = k[A]?[B]° |x L/mol•min Recheck Next (5 of 5) 24th attempt

Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.259 0.549 0.0232 Trial 2 0.518 0.549 0.0928 Trial 3 0.259 1.10 0.0232 Trial 4 0.783 0.210 0.212 Rate = k[A]?[B]° |x L/mol•min Recheck Next (5 of 5) 24th attempt

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

Please help me answer number 2 thank you
Determine the overall rate law for the reaction CH3Br(aq) + OH (aq) → CH3OH(aq) + Br (aq). The data is given below Experiment [CH3B1] (M) [OH"] (M) Initial rate (M/s) k[CH3B1][OH¯]³ O k[CH3B1]°[OH73 1 0.12 0.12 5.2 x 10-5 O k[CH3B1]?[OH"7² 2 0.24 0.12 1.04 x 10-4 O k 3 0.12 0.06 6.5 x 10-6 O KỊCH3B1]°[OH"]) O k(CH3B1]?[OH"]
quickly please
Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.917 0.950 0.252 Trial 2 1.83 0.950 0.504 Trial 3 0.917 1.90 0.504 Trial 4 0.818 0.437 0.103 Rate = k[A]1[B]1
The chemical equation between X and is known to be first order for each reactant. Find the unknown information on the table below.
please answer all as they are part of 1 question but different questions,,.
Excercise 7 please I have done 6
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
O KINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... -1-1 At a certain temperature the rate of this reaction is second order in Cl,0, with a rate constant of 103.Ms: 2Cl,0; (g) 2Cl, (g) +50, (g) → Suppose a vessel contains Cl,0, at a concentration of 0.130M. Calculate the concentration of Cl,0, in the vessel 0.550 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10 Check Explanation Terms of Use | Privacy Center Accessibility 2021 McGraw Hill LLC. All Rights Reserved. II
7:00 Question 13.d of 13 Chemists graph kinetic data to determine rate constants and the order of reactions. Analyze this data. 1 4 7 +/- Given that k is 0.0440 s¹ and the [A] is 0.1000 M, determine the rate for this reaction based on the rate law determined. 2 5 8 Ms™¹ 3 60 Submit 9 O Tap here or pull up for additional resources XU x 100
Show all working explaining detailly your solution. Answer Q13 & 14