ZuoTi.Pro
Question

S2O8^-2(aq)+3I^-(aq)--2SO4^-2(aq)+I3^-(aq) S2O8^-2.        I^-                       rate 0.018M.  &

S2O8^-2(aq)+3I^-(aq)--2SO4^-2(aq)+I3^-(aq)
S2O8^-2.        I^-                       rate
0.018M.         0.018M.             2.6*10^-6
0.018M.         0.036M.             5.3*10^-6
0.072M.         0.036M.             2.12*10^-5

a. write the rate law for this reaction including the reaction order for each reactant
b. calculate the value of k
c. calculate the Rate of the concentration when [S2O8^-2]= 0.2500M and [I]= 0.120M

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
S2O8^-2(aq)+3I^-(aq)--2SO4^-2(aq)+I3^-(aq) S2O8^-2.        I^-                       rate 0.018M.  &
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • (13). if we look to the Rxn: S2O8 (aq)3 1 (aq) 2SO4 (aq) + I3 (aq)...

    (13). if we look to the Rxn: S2O8 (aq)3 1 (aq) 2SO4 (aq) + I3 (aq) 2- We can write the rate of reaction as: Rate=k [S2Os2]1" [I 1" Experimental Data for this Reaction are: Initial Conc.,M Initial rate Expt. [S2Os] [S2Os ]=0.038 [S2Os2= 0.076 S2Os]0.060 [I] Ms RI 1.4 x10 R2=2.8 x10 1 [I]= 0.060 2 [I ]2= 0.060 5 3 [I ]3= 0.120 R3-4.4x10 Find the values m , n and the over all order of reaction?

  • Rate of Disappearance/Rate Constant

    Consider the reaction of peroxydisulfate ion (S2O8^2-)(Aq) with iodide ion (I-) in aqueous solution: (S2O8^2-)(Aq)+(3I-)(Aq)---->2SO4^2-+(I3-)(Aq).At a particular temperature the rate of disappearance of S2O8^2 varies with reactant concentrations in the following manner:Experiment S2O8^2- I- Initial Rate1 0.018 0.036 2.6x10^-62 0.027 0.036 3.9x10^-63 0.036 0.054 7.8x10^-64 0.050 0.072 1.4x10^-51) Determine the rate law for the reaction.Apparently the rate law is Rate=[S2O8^2-][I-]How did they come up with this?2)How is the rate of disappearance ofS2O8^2- related to the rate of disappearance of [I-]...

  • Consider the following reaction: S202(aq)3 I'(aq)2 SO42 (aq) I3 (aq) (a) The rate law for this...

    Consider the following reaction: S202(aq)3 I'(aq)2 SO42 (aq) I3 (aq) (a) The rate law for this reaction is first order in S2O2(aq) and first order in I(aq). What is the rate law for this reaction? k [S02 (aq)] [I(aq)] Rate Rate k [S202-(aq)]2 [r(aq)] Rate k [S20g2-(aq)] [I(aq)]2 Rate k [S2082 (aq )]2 [I°(aq)]12 Rate k [S202(aq)] [I(aq)]3 Rate k [S,02-(aq )]4 [r(aq ) ] (b) If the rate constant for this reaction at a certain temperature is 0.00619, what...

  • Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - )...

    Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - ) in aqueous solution:S2O82 - (aq) + 3 I - (aq)→2 SO42 - (aq) + I3- (aq)At a particular temperature the initial rate of disappearance of S2O8 2 - varies with reactant concentrations in the following manner:Experiment[S2O82‑] (M)[I_] (M)Initial Rate (M/S)10.0180.0362.6 × 10-620.0270.0363.9 × 10-630.0360.0547.8 × 10-640.0500.0721.4 × 10-5(a) Determine the rate law for the reaction and state the units of the rate constant. (b)...

  • 5. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) →...

    5. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M) . [I−](M) . Initial Rate [M/s]    1 0.0300 0.0840 8.80 × 10−4 2 0.0300 0.0420 4.40 × 10−4 3 0.0600 0.0420 8.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction? What is the...

  • 7) The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) →...

    7) The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M)   [I−](M)   Initial Rate [M/s] 1 0.0200 0.0960 7.60 × 10−4 2 0.0200 0.0480 3.80 × 10−4 3 0.0400 0.0480 7.60 × 10−4 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S2O82−][I−] .   ...

  • Preliminary: Key Chemical Equations Reaction 2 Fe3 (a)3 I(a)2 Fe(aq) + I3'(aq) I3(ag) 2 S2032(aq) 3 1a)S4O(0) R...

    Preliminary: Key Chemical Equations Reaction 2 Fe3 (a)3 I(a)2 Fe(aq) + I3'(aq) I3(ag) 2 S2032(aq) 3 1a)S4O(0) Reaction 2: + + Prelab Questions 1. List and define any new terms relevant to this experiment 2. Write the general formula for the rate law for Reaction 1 (given above) 3. Write the general formula for calculating average rate bases on the disappearance of thiosulfate (S2O,2) in Reaction 2 (given above) 4. Write the equation used for calculating a concentration after dilution...

  • For the reaction 2Fe3+ + 3I− ⇆ 2Fe2+ + I3− (all aq); The initial concentrations of...

    For the reaction 2Fe3+ + 3I− ⇆ 2Fe2+ + I3− (all aq); The initial concentrations of Fe3+ and I− are each 0.300 mol/L. The equilibrium concentration of Fe2+ is 0.16 mol/L. Calculate the equilibrium constant, Kc, for this reaction.

  • Consider the reaction, S2O82-   +    3 I-  à    2 SO42-  +  I3-. Data obtained in measuring rate of formation of I3- are...

    Consider the reaction, S2O82-   +    3 I-  à    2 SO42-  +  I3-. Data obtained in measuring rate of formation of I3- are listed in the table. Experiment [S2O82-], M [I‑], M Initial rate, Ms-1 1 0.035 0.055 1.5 x 10-5 2 0.070 0.055 3.0 x 10-5 3 0.070 0.110 6.0 x 10-5 Determine the order of reaction with respect to S2O82-. What is the order of reaction with respect to I-? Give the overall order of reaction. Write the rate law for the reaction. Determine the...

  • Consider the balanced chemical equation. H2O2(aq)+3I−(aq)+2H+(aq)→I3−(aq)+2H2O(l) In the first 14.0 s of the reaction, the concentration...

    Consider the balanced chemical equation. H2O2(aq)+3I−(aq)+2H+(aq)→I3−(aq)+2H2O(l) In the first 14.0 s of the reaction, the concentration of I− drops from 1.000 M to 0.817 M Predict the rate of change in the concentration of H2O2 (Δ[H2O2]/Δt). Express the rate to three significant figures and include the appropriate units. (I understand the arithmetic, but I'm having a tough time with the units)

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT