For the reaction CH₂OH(aq) + H+ (aq) + Cl(aq) → CH₂Cl(aq) + - H₂O(1) the value of [H*] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H* (aq) for the time interval between each measurement. Interval: 0 s to 30.0 s reaction rate: 6.5 X10-3 reaction rate: Incorrect Interval: 30.0 s to 60.0 s 4.8 x10-3 t (s) 0 30.0 60.0 117.0 [H+] (M) 2.34 2.12 2.00 1.83 M/s M/s

For the reaction CH₂OH(aq) + H+ (aq) + Cl(aq) → CH₂Cl(aq) + - H₂O(1) the value of [H] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H (aq) for the time interval between each measurement. Interval: 0 s to 30.0 s reaction rate: 6.5 X10-3 reaction rate: Incorrect Interval: 30.0 s to 60.0 s 4.8 x10-3 t (s) 0 30.0 60.0 117.0 [H+] (M) 2.34 2.12 2.00 1.83 M/s M/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...

See similar textbooks

Similar questions

-1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0482 s H,CO3 (aq) → H,O (aq)+ CO, (aq) Suppose a vessel contains H,CO, at a concentration of 0.300M. Calculate how long it takes for the concentration of H,CO, to decrease by 88.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.260 0.0189 2 0.220 0.520 0.0189 А + 2B → C+ D 3 0.440 0.260 0.0756 Units 0.0484 k M-'s-1 Incorrect
Do not give handwriting solution.
- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M's : 2 NH3 (g) → N, (g)+3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of ammonia. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0045 M's : 2 HI (g) → H, (g)+I, (g) Suppose a 250. mL flask is charged under these conditions with 350. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10
Please answer the question
A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=