{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chemical Kinetics

Chemical Kinetics - Higher concentrations were used in part...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Chemical Kinetics Part one used 2H 2 O 2 (l) 2H 2 O+O 2 to determine the rate law in three experiments with a constant room temperature of 23 degrees Celsius . After graphing each part, the data came out to be fairly linear with a slope with units ml/s. 5ml H2O2 and 10ml KI had a rate of .033 ml/s, solution two with 1ml H2O2 and 10 ml KI had a rate of .058 ml/s, and solution three with 5ml H2O2 and 20 ml KI had a rate of .05 ml/s. In comparison, the different experiments showed to have very similar results because the slopes are very close in quantity. Part two involved the equation 2H 2 O 2 (l) 2H 2 O+O 2 again but with a higher temperature. At 37 degrees Celsius with 10ml KI and 5ml H2O2 the slope for the rate of reaction was .045 ml/s. Thus, the increase in temperature increased the rate. Part three involved allowing the reaction 2H 2 O 2 (l) 2H 2 O+O 2 to go to near completion to prepare for part four where the catalyst is found.
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Higher concentrations were used in part 3 to make the catalyst more apparent. In Part four the solution from part three was titrated in order to retrieve the catalyst. 100% of the catalyst should remain in theory because Ag and I should react 1:1, however only 4.8 x 10-4 of I was found. This could be due to not completely allowing the experiment to go to completion because that would have taken too long. It is also possible that the solution was not completely titrated. Titration was stopped at an orange red color when it is possible that the solution should have been titrated until it reached a blood red color. Also, in part three the warm water slowly decreased closer to room temperature making the temperature not constant. Also, the H2O2 solution could have been oxidized due to the container being exposed to the air after multiple students exposing it....
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online