Homework Answers
we have:
[HI]o = 300 mmol / 4.0 L
= 0.300 mol / 4.0 L
= 7.5*10^-2 M
[HI] = 150 mmol / 4.0 L
= 0.150 mol / 4.0 L
= 3.75*10^-2 M
k = 5.7*10^-3 M/s
use integrated rate law for 0 order reaction
[HI] = [HI]o - k*t
3.75*10^-2 = 7.5*10^-2 - 5.7*10^-3* t
t = 6.579 s
Answer: 6.6 s
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Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0022 M.s: Suppose a 350. mL flask is charged under these conditions with 150. mmol of ammonia. After how much time is there only 75.0 mmol left? 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. x10
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