Asked by Joanaleine Ferrera
A student finds that k = 0.0027 L/mol · s, and m and n are both 1. Calculate the expected rate if 6.0 mL of 0.10 M [S2O82− ] is mixed with 4.0 mL of 0.20 M [I − ]. Assume the final volume of the solution is 10.0 mL.
I used the given molarities and multiplied them by their volumes to find the total moles then I divided by the final volume to get the molarity to multiply with k. Please help!
I used the given molarities and multiplied them by their volumes to find the total moles then I divided by the final volume to get the molarity to multiply with k. Please help!
Answers
Answered by
DrBob222
And what's wrong with multiplying them by k? Looks to me as if you're on the right track.
Answered by
Olereb48
Rate Law with both reactants 1st order:
Rate = (0.0027L/mol-s)[S208^2-][I^-]
[S2O8^2-] = (0.006L)(0.10M)/(0.010L)
= 0.06M
[I^-] = (0.004L)(0.20M)/(0.010L)
= 0.08M
Rate = (0.0027L/mol-s)(0.06mol/L)(0.08mol/L) = 1.3x10^-5 mol/L-s
Rate = (0.0027L/mol-s)[S208^2-][I^-]
[S2O8^2-] = (0.006L)(0.10M)/(0.010L)
= 0.06M
[I^-] = (0.004L)(0.20M)/(0.010L)
= 0.08M
Rate = (0.0027L/mol-s)(0.06mol/L)(0.08mol/L) = 1.3x10^-5 mol/L-s
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.