Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 (CH;),CBr(aq) - (CH3),C (aq) + Br (aq) 2 (CH3),c"(aq) + OH (aq) → (CH3),COH(aq) k2 Suppose als0 k»k. That is, the first step is much faster than the second. O-0 Do Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k O Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for k = 0 the reverse of the two elementary reactions in the mechanism. olo

Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 (CH;),CBr(aq) - (CH3),C (aq) + Br (aq) 2 (CH3),c"(aq) + OH (aq) → (CH3),COH(aq) k2 Suppose als0 k»k. That is, the first step is much faster than the second. O-0 Do Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k O Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for k = 0 the reverse of the two elementary reactions in the mechanism. olo

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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Consider the base hydrolysis of an ester.RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).The kinetics of this reaction, for a particular ester, were studied using the isolation method. When [OH−] << [RCOOR'] a pseudo-rate law can be posed:-d[OH-] / dt = k'' [OH-]mWith initial concentrations: [OH−]0 = 0.0015 M [RCOOR']0 = 0.700 M a plot of ln[OH-] versus t gave a straight line with slope = -0.0176 s-1 and y-intercept = -6.50.What is the order "m"?m = ? What is the corresponding pseudo rate constant k''? (include appropriate units)k'' = ?
For the gas phase decomposition of bromoethane, CH;CH,Br >C,H4 + HBr -1 the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of-2.63x104 K and a y-intercept of 29.6. The value of the rate constant for the gas phase decomposition of bromoethane at 703 K is -1 (Enter your answer to one significant figure.)
provide the given, required, and do the cancellations
0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI
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The reaction for the decomposition of ammonia into its elements is: 2 NH3 (g) → N2 (g) + 3 H2 (g) [N2] 0.0105 M If the concentrations at a certain time are: what will be the associated value of the reaction quotient (Q)? [NH3] = 0.505 M [H2] = 0.414 M, %3D %3D (A) (B) (C) (D) (E) 0.00148 0.00292 0.00861 0.0105 342
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Please solve correctly, find value of x,y,z