Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0026 M·s : 2 HI (g) - H, (g) +L, (g) Suppose a 5.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0026 M·s : 2 HI (g) - H, (g) +L, (g) Suppose a 5.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...
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Transcribed Image Text:Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0026 M.s :
2 HI (g) → H, (g) +I, (g)
Suppose a 5.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 3.0 s later? You may assume no other
reaction is important.
Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
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Expert Solution
Step 1
The rate of the zero-order reaction does not depend on the concentration of the reactant. For the zero-order reaction, the rate constant is given by:
Where [Ao] = initial concentration of the reactant
[At] = concentration of the reactant after t time
k = rate constant of the reaction = 0.0026 M.s-1
t = time = 3.0 s
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