For the isomerization reaction CH3NC (g) → CH3CN (g) in the presence of argon, the rate law is Rate = k[CH3NC]. Experimental measurements at 500 K show that the concentration of reactant has decreased to 75% of its initial value after 440 seconds. How much additional time will be required for the concentration of CH3NC to drop to 25% of its initial value? E) 440 A) 2120 B) 1680 C) 1320 D) 880

For the isomerization reaction CH3NC (g) → CH3CN (g) in the presence of argon, the rate law is Rate = k[CH3NC]. Experimental measurements at 500 K show that the concentration of reactant has decreased to 75% of its initial value after 440 seconds. How much additional time will be required for the concentration of CH3NC to drop to 25% of its initial value? E) 440 A) 2120 B) 1680 C) 1320 D) 880

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

20
A) In the proposed reaction mechanism below, the intermediate product is: A). NO(g) B). N2O2(g) C). H2(g) D). N2O(g) B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors A) 2 B) 3 C) 6 D) 9
The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?
The rate for the overall reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) is Rate = k[NO2]2 a. Consider this mechanism: i. 2NO2 (g) → N2 (g) + 2O2 (g) [slow] ii. 2CO (g) + O2 (g) → 2CO2 (g) [fast] iii. N2 (g) + O2 (g) →2NO (g) [fast] d. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0019 M/s. What rate is the molecular oxygen being consumed?
4 At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 6.83 × 10 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.890M. Calculate the concentration of CICH₂CH₂Cl in the vessel 880. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0022 M/s. What rate is the molecular oxygen being consumed?
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider the following fictitious reaction and the measured initial rates at different reaction conditions. Determine the rate law for this reaction. X (g) + y (g) XY (g) Trial 1 2 3 Initial Rate (M/h) 0.05069 [X] M [Y] M 0.1383 0.1860 0.1383 0.6783 0.18476 0.3804 0.1860 0.05079
Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0019 M/s. What rate is the molecular oxygen being consumed?