Consider the second-order reaction: 2HI(g)→H₂(g) + 1₂ (8) Use the simulation to find the initial concentration [HI] and the rate constant & for the reaction. What will be the concentration of HI after t=5.44x100 s ([HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters three significant figures. ▸ View Available Hint(s) for Part B for Brat do for Part [HI] 1.68 10 -3 Submit Previous Answers redo foart Breor Part B keyboard shortcuts for Part B help for Part B X Incorrect; Try Again; 5 attempts remaining mol

Consider the second-order reaction: 2HI(g)→H₂(g) + 1₂ (8) Use the simulation to find the initial concentration [HI] and the rate constant & for the reaction. What will be the concentration of HI after t=5.44x100 s ([HI],) for a reaction starting under the condition in the simulation? Express your answer in moles per liters three significant figures. ▸ View Available Hint(s) for Part B for Brat do for Part [HI] 1.68 10 -3 Submit Previous Answers redo foart Breor Part B keyboard shortcuts for Part B help for Part B X Incorrect; Try Again; 5 attempts remaining mol

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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1/(a。 - x) Slope=-0.0725 Intercept= 66.7 time calculate the rate constant of the reaction. O Cannot be determined O +0.0376 Ⓒ -0.0752 -0.0376 +0.0752
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Pallles A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [] Initial rate of reaction 1.60 M 2.25 M 19.0 M/s 3.17 M 2.25 M ||Mis 0.727 M 4.95 M |Mis Check Save For Later Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility EPIC 8. MacBook Pro esc F2 F3 F4 F5 F6 F7 F8 F12 OLd # 3 2$ 4. * % de 7. 6. 5. 9. 国国国 00 E881E R. } tab E. aps lock K. 国国5 C 己 W. alt control option command command option
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Current Attempt in Progress The following reaction is investigated to determine its rate law: 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-) [NO) [H,1 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10- 0,80 x 10-4 0.60 x 10-4 8.0 x 10- What is the rate law for the reaction? O rate = k [NO][H2]² O rate = k [NO]?[H2] O rate = k (NO]?[H2]? O rate = k (NO][H2] What is the value of the rate constant? k= i x 105 O L mol 1s1 O s-1 O L³mol 3s1 O mol L1s-1 O L² mol-2s 1
1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth
Question 17 of 23 Submit Butadiene reacts to form a dimer according to the equation 2C,H6(g) → C3H12(g) The reaction obeys the second order rate law, Rate = k[C,H,]?, with a rate constant k = 3.68 M-'min at a certain temperature. Starting with an initial concentration of [C,H] = 0.0500 M, what will be the butadiene concentration after 31.0 min? | M 1 2 3 C 7 9. +/- x 10 0 LO 00
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