ZuoTi.Pro
Question

Consider the reaction : 2MnO4- + 5H2O2 + 6H+ --> 2Mn2+ +5O2 +8H2O. If it takes...

Consider the reaction : 2MnO4- + 5H2O2 + 6H+ --> 2Mn2+ +5O2 +8H2O. If it takes 36.44 mL of 0.01652 M KMnO4 solution are required to oxidize 25.00 mL of a H2O2 solution, Calculate the molarity of the H2O2 solution.State your final answer using 4 Sigfigs.

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

Homework Answers

Answer #1

from given equation,
2 moles of KMnO4 reacts with 5 moles of H2O2

so,
moles of H2O2 required = (5/2)* moles of KMnO4
M(H2O2)*V(H2O2) = (5/2)*M(KMnO4)*V(KMnO4)
M(H2O2) * 25.00 = (5/2)*0.01652 * 36.44
M(H2O2) = 0.06020 M
Answer: 0.06020 M

0 0
Add a comment
Know the answer?
Add Answer to:
Consider the reaction : 2MnO4- + 5H2O2 + 6H+ --> 2Mn2+ +5O2 +8H2O. If it takes...
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

  • For the reaction 5H2O2 + 2MnO4- + 6H+ ----> 2Mn2+ + 5O2 + 8H2O

    For the reaction 5H2O2 + 2MnO4- + 6H+ ----> 2Mn2+ + 5O2+ 8H2O, the experimentally dtermined rate of disappearance of MnO4-is 2.2x10-3 M/s. Calculate the reaction rate.

  • For the reaction 5H2O2 + 2MnO4- + 6H+ → 2Mn2+ +5O2 + 8H2O

    For the reaction 5H2O2 + 2MnO4- + 6H+ → 2Mn2+ +5O2 + 8H2O•The experimentally determined rate of disappearance of MnO4- is 2.2x10-3 M/s •Write out the relative rates for all chemicals involved in the reaction.

  • For the reaction 5H2O2 + 2MnO4- +6H+ → 2Mn2+ +5O2 + 8H2O

    For the reaction 5H2O2 + 2MnO4- +6H+ → 2Mn2+ +5O2 + 8H2O The experimentally determined rate of disappearance of MnO4 is 2 2x10-3 M/s. Calculate the reaction rate. Enter the value only. The units of the value you enter wanted to enter the value 0.063, enter either 0.063 or 6.3E-2. 

  • The concentration of hydrogen peroxide solution can be determined by titration against a standardized solution or...

    The concentration of hydrogen peroxide solution can be determined by titration against a standardized solution or potassium permanganate in acidic medium according to the following equation: 2MnO4 + 5H2O2 + 6H* -----> 502 + 2Mn+2 + 8H2O What is being oxidized? What is being reduced? What is the oxidizing agent? What is the reducing agent? If 36.44 mL of a 0.01652 M KMnO4 solution are required to oxidize 25.00 mL of a H2O2 solution, calculate the molarity of the H2O2...

  • Consider the following two reactions involving oxalic acid. 2MnO4− + 5H2C2O4 + 6H+ → 2Mn2+ +...

    Consider the following two reactions involving oxalic acid. 2MnO4− + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2 + 8H2O H2C2O4 + 2OH− → C2O42− + 2H2O What volume of 0.0100 M KMnO4 solution will titrate a solution prepared from 46.0 mg of H2C2O4? What volume of 0.0100 M NaOH solution will titrate a solution prepared from 46.0 mg of H2C2O4?

  • The redox reaction between hydrogen peroxide, H2O2, and permanganate ions, MnO4-, in acid solution are as...

    The redox reaction between hydrogen peroxide, H2O2, and permanganate ions, MnO4-, in acid solution are as follows: 5H2O2(aq) + 2MnO4-(aq) + 6H+(aq)  →   5O2(g) + 2Mn2+(aq) + 8H2O (l) 5 mol of MnO4-was required to reach the equilibrium. How many moles of H2O2were required to reach the equilibrium? a) 2 mol                            b. 10 mol c) 12.5 mol            d) 25 mol

  • A permanganate solution is standardized by titrating it with a 0.1491 M hydrogen peroxide solution. The...

    A permanganate solution is standardized by titrating it with a 0.1491 M hydrogen peroxide solution. The balanced net ionic equation for the reaction is: 2MnO4-(aq) + 5H2O2(aq)+6H3O+(aq)2Mn2+(aq) + 5O2(g)+14H2O(l) If 21.22 mL of the 0.1491 M hydrogen peroxide solution is required to react completely with 25.00 mL of the permanganate solution, calculate the concentration of the permanganate solution.

  • QUESTION 11 Given the following balanced chemical reaction: 2MnO4 (aq) + 5NO2 (aq) + 6H* (aq)...

    QUESTION 11 Given the following balanced chemical reaction: 2MnO4 (aq) + 5NO2 (aq) + 6H* (aq) -- 2Mn2(aq) + NO3(aq) + 3H20 (1) 25.0 mL of an aqueous Mo(MnO4)2 solution is titrated with a 0.137M A(NO2)3 solution. If it requires 35.5 mL of the Al(NO2)2 solution to completely react with the Mg(MnO4)2 solution, what is the molarity of the original Mg(MnO4)2 solution? 0.0780 M 0.00292 M 0.117M 0.00584 M 0.234 M

  • can you please answer this one, the first one I posted the answer was wrong. Potassium...

    can you please answer this one, the first one I posted the answer was wrong. Potassium permanganate in acidic solution is used to titrate a solution of hydrogen peroxide, with which it reacts according to 2MnO4 (aq) + 5H2O2(aq)+6H30+(aq)—>2Mn2+(aq) + 502(g)+14H2O(1) A potassium permanganate solution is prepared by dissolving 22.00 g of KMnO4 in water and diluting to a total volume of 1.000 L. A total of 20.27 mL of this solution is required to reach the endpoint in a...

  • 1. Calculations Given the following data, determine the % by mass of oxalate (C2O42-) in a...

    1. Calculations Given the following data, determine the % by mass of oxalate (C2O42-) in a sample of an iron oxalate complex with the general formula Kz[Fex(C2O4)y].wH2O. The reaction between oxalate and permanganate is as follows: 6H+ + 5(COOH)2 + 2MnO4- → 10CO2 + 2Mn2+ + 8H2O m(iron oxalate complex) used for titration = 0.100 g C(KMnO4) standard solution = 0.0200 M M(C2O42-) = 88.02 g mol-1 Titre volume = 10.18 mL Enter your answer to 3 significant figures. 2....

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