🤓 Based on our data, we think this question is relevant for Professor Keyes' class at BU.
The thiosulfate ion (S2O32-) is oxidized by iodine as follows:
2S2O32- (aq) + I2 (aq) → S4O62- (aq) + 2I - (aq)
In a certain experiment, 7.05 x 10-3 mol/L of S2O32- is consumed in the first 11.0 seconds of the reaction. Calculate the rate of consumption of S2O32-. Calculate the rate of production of iodide ion.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Average Rate of Reaction concept. You can view video lessons to learn Average Rate of Reaction. Or if you need more Average Rate of Reaction practice, you can also practice Average Rate of Reaction practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Keyes' class at BU.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.