Investigating the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid

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... ivided the light depreciation (k lux) by the time taken (minutes) to give a rate of k lux/min. Light depreciation is k lux at start minus k lux at end of reaction. Here are the results:

Graph

Reaction Finished in

k lux at start

k lux at end

k lux dep./s

DPPAS_02

70s

8.9

2.1

.097

DPPAS_03

80s

8.9

2.7

.078

DPPAS_04

100s

8.4

3.2

.052

DPPAS_05

N/A

8.3

N/A

N/A

Analysis / Conclusion : Our results show that, as predicted, the more concentrated solutions reacted more quickly than the weaker ones. As the concentration got weaker, the reaction was slower. I would expect the same pattern of you swapped Sodium Thiosulphate and Hydrochloric Acid for two other chemicals, which are not affected by water, but will react with each other. There were a few anomalies at the beginning of two of our graphs, but the end results were all in proportion. The experiment shown in DPPAS_02 twice as conc ...

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