For the reaction
5H2O2 + 2MnO4- + 6H+ ----> 2Mn2+ + 5O2+ 8H2O, t
he 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•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 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.
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.
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
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?
(As soon as possible) Balance each of the following equations according to the half-reaction method: H2O2(aq) + MnO4−(aq)⟶Mn2+(aq) + O2(g) (in acid) 5H2O2(aq) + MnO4−(aq) + 6H3O+(aq) ⟶ Mn2+(aq) + 5O2(g) + 14H2O(l) 5H2O2(aq) + 2MnO4−(aq) + 6H3O+(aq) ⟶ 2Mn2+(aq) + 5O2(g) + 14H2O(l) 5H2O2(aq) + 2MnO4−(aq) + 7H3O+(aq) ⟶ Mn2+(aq) + 5O2(g) + 15H2O(l)
(b) What is E°cell for the reaction 2MnO4- + 16H+ + 5Pb → 5Pb2+ + 2Mn2+ + 8H2O?
2Mn2+ +5H3AsO4⇌5HAsO2+2MnO4-+ 6H++ 2H2OIn the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.2Cl2 +5Sb2O5+ 6H+ ⇌10SbO++4ClO3-+ 3H2OIn the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.2MnO4-+3N2H4+ 4H2O⇌6NH2OH+ 2MnO2+ 2OH-In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.
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
Rate equation is rate =
k[MnO4-]x[H2C2O4]y
Understand what [MnO4-],
[H2C2O4], x, y and k are. How to
calculate the x,y, and k in this experiment?
2Mno4-+5H2C2O4+6H+2Mn2++10CO2+8H2O