3499qpqThe gas phase decomposition of hydrogen iodide at 700 KHI(g) → H₂(g) + % 1₂ (9)is second order in HI with a rate constant of 1.20 × 10-³ 1M-sIf the initial concentration of HI is 0.610 M, the concentration of HI will beSubmit AnswerRetry Entire Group4 more group attempts remainingM after 3330 seconds have passed. The gas phase decomposition of hydrogen iodide at 700 KHI(g) → H₂(g) + ½ 1₂ (9)is second order in HI with a rate constant of 1.20 x 10-³1M-sIf the initial concentration of HI is 2.27 M, the concentration of HI will be 0.377 M after |Submit AnswerRetry Entire Group 4 more group attempts remainingseconds have passed.

Answered: Image /qna-images/answer/48b58ae4-7160-4ee3-9544-81ef24c6a313.jpg

The gas phase decomposition of hydrogen iodide at 700 K HI(g) → H₂(g) + % 1₂ (9) is second order in HI with a rate constant of 1.20 x 10-³ 1 M-s If the initial concentration of HI is 2.27 M, the concentration of HI will be 0.377 M after Submit Answer Retry Entire Group 4 more group attempts remaining seconds have passed.

The gas phase decomposition of hydrogen iodide at 700 K HI(g) → H₂(g) + % 1₂ (9) is second order in HI with a rate constant of 1.20 x 10-³ 1 M-s If the initial concentration of HI is 2.27 M, the concentration of HI will be 0.377 M after Submit Answer Retry Entire Group 4 more group attempts remaining seconds have passed.

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

A reaction is second order with respect to reactant "A" and has a rate constant of 2.97 x 10-2 M-1s-1. If the initial concentration of A is 0.100 M, what will the concentration drop to after 30.0 minutes? 6.06 x 10E(-25) M 9.18 x 10E(-2) M 1.58 x 10E(-2) M 1.01 x 10E(-26) M
For the reaction 2A → 2B + C, it was found to be 1st order. How long will it take for the concentration to go from 0.0159 M to 0.0062 M, if the rate constant is 0.017 s1? Answer to 1 decimal place.
The gas phase decomposition of nitrogen dioxide at 383 °C NO₂ (g) → NO(g) + ½/0₂ (9) is second order in NO₂ with a rate constant of 0.540 1 M.S If the initial concentration of NO₂ is 0.485 M, the concentration of NO2 will be M after 16.5 seconds have passed.
Use the References to access important values if needed for this question. The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)→NO(g) + ½ Cl2(g) is second order in NOCI with a rate constant of 5.90×10-4 M¯ls1 If the initial concentration of NOCI is 8.28×10 2 M, the concentration of NOCI will be M after 4.82×104 seconds have passed.
A decomposition reaction follows second order kinetics with a rate constant, k = 0.0137 M-1 min-1. If the initial concentration of the reactant is 0.866 M, what is the concentration after 5 minutes? Report your answer to the thousandths place and do not include units.
The decomposition of nitrosyl bromide at 10 °C NOBrNO +2 Br₂ is second order in NOBr with a rate constant of 0.800 1 M.S If the initial concentration of NOBr is 0.228 M, the concentration of NOBr will be 4.86 x 10-2 M after I Submit Answer seconds have passed. Retry Entire Group 8 more group attempts remaining
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 0.210 0.0157 A + 2B C+D 0.220 0.420 0.0157 3 0.440 0.210 0.0628 Units k = M-ls-1 M-2s-1 M-s-1
The rate law for the reaction A2BM2(aq) + 2A(aq) + 2D(aq) → D2(aq) + 2A½Bm (aq) is rate = k(A2Bm2)(D). %3D What is the overall order of the reaction? O zeroth order O first order third order second order
Don't give handwritten answers otherwise I will dislike
The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.
Solve it asap
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.260 0.280 0.0119 A + B → C+ D 2 0.260 0.784 0.0933 3 0.312 0.280 0.0143 Units k = M-²s-1 M-'s-! M-s-!