Stiller2- (a) At some point in the reaction 2A +B G + 3H, [A]=0.3629 M. At a time 8.25 minlater [A] = 0.3187 M. What is the average rate of formation of H during this time interval,expressed in M/s?(b) The first order decomposition reaction of N2Os is given as follows;N2O5 (in CCL) → N»O4 (in CCL) + ½ 02(g)Find the rate constant (k) corresponding to a 2.00 h half-life at 25°C. Calculate the half-life ofthe given decomposition reaction at 32°C, if the activation energy is 106 kJ/mol? (R:8.314J/mol K)

Given, The concentration of A is 0.3629 M. The concentration of A after time interval is 0.3187 M.

2- (a) At some point in the reaction 2A + B G+ 3H, [A]=0.3629 M. At a time 8.25 min later [A] = 0.3187 M. What is the average rate of formation of H during this time interval, %3D expressed in M/s? (b) The first order decomposition reaction of N2O5 is given as follows; N2O5 (in CCL) → N»O4 (in CCL4) + ½ O2(g) Find the rate constant (k) corresponding to a 2.00 h half-life at 25°C. Calculate the half-life of the given decomposition reaction at 32°C, if the activation energy is 106 kJ/mol? (R:8.314 J/mol.K)

2- (a) At some point in the reaction 2A + B G+ 3H, [A]=0.3629 M. At a time 8.25 min later [A] = 0.3187 M. What is the average rate of formation of H during this time interval, %3D expressed in M/s? (b) The first order decomposition reaction of N2O5 is given as follows; N2O5 (in CCL) → N»O4 (in CCL4) + ½ O2(g) Find the rate constant (k) corresponding to a 2.00 h half-life at 25°C. Calculate the half-life of the given decomposition reaction at 32°C, if the activation energy is 106 kJ/mol? (R:8.314 J/mol.K)

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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