Question

The rate law for the iodine-clock reaction: Rate = k[I-]a[BrO3]b[H+]c Solve for k and write the units. 4.03x10^-7 M/s = k (0.00167M)^1(0.00667M)^1(0.0167M)^2

Name: the rate law for the iodine clock reaction rate ki abro3bhc solve for k and write the units 403x10 7 ms k 000167m1000667m100167m2 30963
Uploaded: 2023-01-27T18:30:12-08:00
Duration: 2 min 6 s
Channel: David Collins
Description: the rate law for the iodine clock reaction rate ki abro3bhc solve for k and write the units 403x10 7 ms k 000167m1000667m100167m2 30963

          The rate law for the iodine-clock reaction:
Rate = k[I-]a[BrO3]b[H+]c
Solve for k and write the units.
4.03x10^-7 M/s = k (0.00167M)^1(0.00667M)^1(0.0167M)^2

Added by Shane B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

01/27/2023

Step 1

The rate law is given as: \[ \text{Rate} = k[I^-]^a[BrO_3^-]^b[H^+]^c \] The provided values are: - Rate = \(4.03 \times 10^{-7} \, \text{M/s}\) - \([I^-] = 0.00167 \, \text{M}\) - \([BrO_3^-] = 0.00667 \, \text{M}\) - \([H^+] = 0.0167 \, \text{M}\) Show more…

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The rate law for the iodine-clock reaction: Rate = k[I-]a[BrO3]b[H+]c Solve for k and write the units. 4.03x10^-7 M/s = k (0.00167M)^1(0.00667M)^1(0.0167M)^2