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Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0070 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0070 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 1RQ: Define reaction rate. Distinguish between the initial rate, average rate, and instantaneous rate of...
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- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0070 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 2.0 s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ar x10
Transcribed Image Text:- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0070 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 2.0 s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ar x10
Expert Solution
Step 1

A zero order reaction is the independent of the reactant concentration.

And formula used

[A]t = - kt + [A]0

Where [A]t is concentration of HI after 2.0 s.

k = rate constant = 0.0070 M.s-1 .

and t = time = 2.0 s; and

[A]0 = Initial concentration of HI = 100.0 × 10-3 moles / 2.0 L = 0.05 M

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