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# The order of the decomposition of hydrogen peroxide

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Introduction

The order of the decomposition of hydrogen peroxide Objectives: To show that the decomposition of hydrogen peroxide is a first order reaction Introduction: Refer to the lab manual Apparatus: Refer to the lab manual Chemicals: Refer to the lab manual Procedures: Refer to the lab manual Precautions: Refer to the lab manual Results: Time /min Final burette reading /cm3 Initial burette reading /cm3 Volume of KMn04 /cm3 0 41.20 10.80 30.40 5 25.20 1.15 ...read more.

Middle

time t, the concentration of hydrogen peroxide at these times are proportional to Vo and Vt respectively t /min a, Vo /cm3 a-x, Vt /cm3 x, Vo-Vt /cm3 log a/(a-x) k = (2.303/t)[ log a/(a-x)] 0 30.40 30.40 0 0 / 5 30.40 24.05 6.35 0.102 0.0469 10 30.40 18.35 12.05 0.219 0.0505 15 30.40 14.85 15.55 0.311 0.0478 20 30.40 11.85 18.55 0.409 0.0471 25 30.40 9.05 21.35 0.526 0.0485 30 30.40 7.05 23.35 0.635 0.0487 bi. ...read more.

Conclusion

- 0.0362(2)(12) + 1.4988 = 0.803 cm3min-1 Vt at t = 8mins = -0.0004 (83) + 0.0362 (82) - 1.4988(8) + 30.456 = 20.58 cm3 Vt at t = 12mins = -0.0004 (123) + 0.0362 (122) - 1.4988(12) + 30.456 = 16.99 cm3 0.996 = k(20.58)n -----(1) 0.803 = k(16.99)n -----(2) logk = (log0.803log20.58 - log0.996log16.99)/(log20.58 - log16.99) k = 0.0328 d. Yes, they do. The graph (iii) shows a straight line. e. t1/2 from graph (i) from graph (ii) a to a/2 14.35 a/2 to a/4 28.60 a/4 to a/8 ...read more.

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