Cliffs AP Chemistry, 3rd Edition

Order with respect to H 2 O 2 = First order according to Graph for Part 2

X = 1st order = 0.6107 *slope = order = x

[H 2 O 2 ] log [H 2 O 2 ] Time, sec Rate Log rate

0.04 −1.397940009 47 1.06383 × 10 –05 −4.973127854

0.03 −1.5228 78745 51 9.80392 × 10 –06 −5.008600172

0.022 −1.657577319 60 8.33333 × 10 –06 −5. 07 91812 4 6

0.018 −1.744727495 70 7.14286 × 10 –06 −5.146128036

0.014 −1.853871964 90 5.55556 × 10 –06 −5.255272505

Part III. Reaction Order with Respect to Hydronium Ion

Beaker A Beaker B

0.05 KI [I–] 0.05M Buffer 2 0.1 M [H 2 O 2 ] Time Initial Partial

(mL) (M) Na 2 S 2 O 3 (mL) H 2 O 2 (M) (s) rate Order

(mL) (mL) (M/s)

10.0 0.010 1.0 19.0 20.0 0.040 45 1 .11111 × 10 –5 0.037761

10.0 0.010 1.0 24.0 15.0 0.030 50 1.00000 × 10 –5 0.0172

10.0 0.010 1.0 28.0 11.0 0.022 75 6.66667 × 10 –6 −0.193819

10.0 0.010 1.0 30.0 9.0 0.018 104 4.80769 × 10 –6 −0.34387

10.0 0.010 1.0 32.0 7.0 0.014 130 3.84615 × 10 –6 −0.31940

Average order with respect to H 3 O+= 0.1604256 Zero order

Graph for Part 2

log [H 2 O 2 ]

log rate y = 0.6107x − 4.0937

log rate

linear (log rate)

-2 -1.5 -1 -0.5 0

-4.9

-5

-5.1

-5.2

-5.3

Laboratory Experiments