In a study of the reaction of pyridine (C;H;N) with methyl iodide (CH;I) in a benzene solution, the following set of initial reaction rates was measured at 25°C for different initial concentrations of the two reactants: [C,H;N] (mol L1) [CH;I] (mol L-) Rate (mol Ls') 1.00 x 10-4 1.00 x 10-4 7.5 x 10-7 2.00 x 10-4 4.00 x 10-4 2.00 x 10-4 3.0 x 10- 2.00 x 10-4 6.0 x 10-6 (a) Write the rate expression for this reaction. (b) Calculate the rate constant k and give its units. (c) Predict the initial reaction rate for a solution in which [C;H;N] is 5.0 × 10-5 M and [CH;I] is 2.0 × 10-5 M.

In a study of the reaction of pyridine (C;H;N) with methyl iodide (CH;I) in a benzene solution, the following set of initial reaction rates was measured at 25°C for different initial concentrations of the two reactants: [C,H;N] (mol L1) [CH;I] (mol L-) Rate (mol Ls') 1.00 x 10-4 1.00 x 10-4 7.5 x 10-7 2.00 x 10-4 4.00 x 10-4 2.00 x 10-4 3.0 x 10- 2.00 x 10-4 6.0 x 10-6 (a) Write the rate expression for this reaction. (b) Calculate the rate constant k and give its units. (c) Predict the initial reaction rate for a solution in which [C;H;N] is 5.0 × 10-5 M and [CH;I] is 2.0 × 10-5 M.

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

nder [reactant), Treactant]," rate, rate; What is the reaction order with respect to A? (A), mol/L (B), mol/L rate, mol/(L-min) Trial 1 0.931 0.549 0.0781 Trial 2 1.86 0.549 0.0781 Trial 3 0.931 1.10 0.312 Trial 4 0.466 0.829 0.178 Rate = k(A]ordera B]arderb 2
5 Br-(aq) + BrO3-(aq) + 6 H+(aq)--> 3 Br2(aq) + 3 H2O(l); (a) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)
A+OHA+H₂O O₂ (g) ⇒ 0₂ (soln) O₂ (soln) + X⇒ B B + A⇒X+ products (fast equilibrium) (fast) (fast) (slow) Show that the observed rate law: d[products]/dt = kobs[B][A][OH]. Include step-by-step solution.
None
Writing the rate law of an elementary reaction Write the rate law for the following elementary reaction: 2 N,O5(g) → 2 N,04(9) + O2(g) Use k, to stand for the rate constant. rate ? olo ||
3 - Consider the gas phase decomposition of acetic acid at 1200 K. It proceeds via two parallel reactions: CH:COOH → CH+ + CO: ki = 3.74 s CH:COOH – CH:co + H2O k2 = 4.65 s'! (a) What is the maximum percentage yield of the ketene CH:CO at this temperature? (b) What is the concentration of the ketene when the extent of reaction when is 0.5 (50%)? (c) To favor the second reaction, should you increase or decrease temperature?
Obtain the 2"-1 – 1 | T (п - 1)k. а"-1 relation between the order of the reaction (n), the reaction rate constant (k), the initial concentration (a), and the half-life (T).
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'' = ?
14.17 What is Kp at 1273°C for the reaction 2CO(g) + O2(8) = 2CO2(g) if K. is 2.24 × 10“ at the same temperature?
The following experimental data were obtained for the reaction of NH,+ and NO2- in acidic solution. NH, + (aq) + NO2 (aq) → N2 (g) +2 H2O(€) [NH, ] (mol L) NO, ¯] (mol L1) Rate = A[N2]/At (mol L-s) 0.0096 0.110 3.06 x 10-7 0.0096 0.055 1.53 x 10-7 0.0509 0.220 3.25 x 10-6 0.0259 0.220 1.65 x 10-6 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =| mol L-1s 1 Try s1 L mol-1 s-1 L² mol-2 Submit Answer 9 item attempts remaining
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?
please help me with question a and b only