In a study of the decomposition of ammonia on a platinum surface at 856 °CNH3-1/2 N₂ + 3/2 H₂the following data were obtained:[NH3], Mseconds5.79x10-302.90x10-39981.45x10-3 7.25x10-41.50x10³ 1.75x103Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 5.79x10-³ M isstarting concentration is 2.90x10-³ M isS.(2)The average rate of disappearance of NH3 from t = 0 s to t = 998 s is(4)Based on these data, the rate constant for this(3)The average rate of disappearance of NH3 from t = 998 s to t = 1.50x10³ s isorder reaction isM s ¹.M S-1Ms¹.s and when the

Answered: In a study of the decomposition of…

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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In a study of the decomposition of ammonia on a platinum surface at 856 °C
NH3-1/2 N₂ + 3/2 H₂
the following data were obtained:
[NH3], M
seconds
5.79x10-3
0
2.90x10-3
998
1.45x10-3 7.25x10-4
1.50x10³ 1.75x103
Hint: It is not necessary to graph these data.
(1)
The observed half life for this reaction when the starting concentration is 5.79x10-³ M is
starting concentration is 2.90x10-³ M is
S.
(2)
The average rate of disappearance of NH3 from t = 0 s to t = 998 s is
(4)
Based on these data, the rate constant for this
(3)
The average rate of disappearance of NH3 from t = 998 s to t = 1.50x10³ s is
order reaction is
M s ¹.
M S-1
Ms¹.
s and when the

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“Since you have posted a question with multiple sub-parts, we will solve the first three subparts for you. To get the remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.”

Finding the order of the reaction is the first step in solving this issue. The other components will then be resolved using the integrated rate law of that order of the reaction. The units of the rate constant can also be used to determine the order of the reaction.

For a zero-order reaction, the unit for the rate constant is given by = M/s

For a first-order reaction, the unit for the rate constant is given by= s^-1

For a second-order reaction, the unit for the rate constant is given by M^-1s^-1

A zero-order reaction's rate constant, M/s, was mentioned as part of our problem's fourth section. Therefore, zero-order kinetics will be used to address our issue.

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