Reaction Order and Rate Laws
Hands-On Labs, Inc.
Version 42-0195-00-02 Lab Report Assistant
This document is not meant to be a substitute for a formal laboratory report. The Lab Report
Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data
tables that should be addressed in a formal lab report. The intent is to facilitate students’
writing of lab reports by providing this information in an editable file which can be sent to an
instructor. Exercise 1: Determining the Rate Laws of the Reaction
between HCl and Na2S2O3
Data Table 1. Varying Concentrations of 1.0 M HCl.
Concentrations
# of # of
drops drops # of
Stock
Stock
drops Solution Solution Reaction Reaction
(after
mixing in
well) HCl (after
mixing in
well) Reaction Time
(seconds) Well # HCl H2O Na2S2O3 HCl Na2S2O3 C1, D1 12 0 8 1M 0.3M 34 36 52 C2, D2 6 6 8 1M 0.3M 50 52 77 C3, D3 4 8 8 1M 0.3M 62 68 96 Reaction
Rate
(sec-1) Na2S2O3 Trial 1 Trial 2 Average Data Table 2. Varying Concentrations of 0.3 M Na2S2O3.
Concentrations
# of # of
drops drops # of
Stock
Stock
drops Solution Solution Reaction Reaction
(after
mixing in
well) HCl (after
mixing in
well) Reaction Time
(seconds) Well # HCl H2O Na2S2O3 HCl Na2S2O3 Na2S2O3 Trial 1 Trial 2 Average C4, D4 8 0 12 1M 0.3M 24 26 25 C5, D5 8 6 6 1M 0.3M 48 46 47 C6, D6 8 8 4 1M 0.3M 80 86 83 Reaction
Rate
(sec-1) Questions
A. Determine the Reaction Order for HCl using calculations described in the Background
section. Show your work. Note that your answer will probably not be an even whole
number as it is in the examples, so round to the nearest whole number. B. Determine the Reaction Order for Na2S2O3 using calculations described in the Background
section. Show your work. Note that your answer will probably not be an even whole
number as it is in the examples. C. Write the rate law for the reaction between HCl and Na2S2O3. D. Using the following rate law, and the experimental values given, calculate k: Rate = k[F2][ClO2]
Experiment
1
2
3
E. [F2] (M)
0.5
0.8
0.5 [ClO2] (M)
0.5
0.8
0.8 Initial rate (M/s)
0.300 M/s
0.768 M/s
0.480 M/s Describe sources of error in this experiment?
The sources of error for this experiment could have been with not adding the right
amounts in the solutions as well as that of contamination in the wells that were used to
hold the solutions that were being tested.

• 1503237812-CHM151r2_Reaction_Order_and_Rate_Laws_Lab_Assistant.docx

AccountingQueen

(3)

Status NEW Posted 20 Aug 2017 02:08 PM My Price 10.00

Hel-----------lo -----------Sir-----------/Ma-----------dam----------- T-----------han-----------k y-----------ou -----------for----------- us-----------ing----------- ou-----------r w-----------ebs-----------ite----------- an-----------d a-----------cqu-----------isi-----------tio-----------n o-----------f m-----------y p-----------ost-----------ed -----------sol-----------uti-----------on.----------- Pl-----------eas-----------e p-----------ing----------- me----------- on----------- ch-----------at -----------I a-----------m o-----------nli-----------ne -----------or -----------inb-----------ox -----------me -----------a m-----------ess-----------age----------- I -----------wil-----------l

Not Rated(0)

• Buy Answer