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.
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•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.
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
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
A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2MnO4-(aq) + 16H+(aq) + 5Pb(s) -> 2Mn2+(aq) + 8H2O(l) + 5Pb2+(aq) Suppose the cell is prepared with 2.08M MnO4- and 1.77M H+ in one half-cell and 1.82M Mn2+ and 1.13M Pb2+ in the other. Calculate the cell voltage under these conditions. Do not round intermediate calculations. Round your answer to 3 significant digits.
A solution containing 0.190.19 M Pb2+Pb2+ , 1.5×10−61.5×10−6 M Pb4+Pb4+ , 1.5×10−61.5×10−6 M Mn2+Mn2+ , 0.190.19 M MnO−4MnO4− , and 0.900.90 M HNO3HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+]5[Pb4++2e−↽−−⇀Pb2+] ?∘+=1.690 VE+°=1.690 V 2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O]2[MnO4−+8H++5e−↽−−⇀Mn2++4H2O] ?∘−=1.507 VE−°=1.507 V 5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16H+5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO4−+16H+ A. Determine ?∘cellEcell∘, Δ?∘ΔG∘, and ?K for this reaction. ?∘cell=Ecell∘= V Δ?∘=ΔG∘= J ?=K= B. Calculate the value for the cell potential, ?cellEcell, and the free energy, Δ?ΔG, for the given conditions....
1. Potassium permanganate (KMnO4 ) is a commonly used oxidant in many redox titrations. In one such titration, KMnO4 solution in a buret is added to a solution of oxalic acid in the Erlenmeyer flask. 2MnO4−(aq) + 5H2C2O4(aq) + 6H+(aq) → 2Mn2+(aq) + 10 CO2(g) + 8 H2O(l) Every component except permanganate (purple) is colorless. The end point of the reaction will be signaled by: a. The first appearance of the purple color in the solution being titrated b. The...
2) Consider the reaction: 8H2S(g) + 402(g) → 8H2O(g) + S8(g) Complete the table including units, Show your work below. A[H2S]/At A[02]/At A[H20]/At A[S2]/At Rate -0.080 M/S
The rate of a chemical reaction can be measured as the rate of appearance of any of the products or as the rate of disappearance of any of the reactants. These relative rates of reaction are related through the stoichiometry of the overall reaction. For example, the rate of the reaction shown below can be determined by measuring the initial rate of disappearance of I, -A[I/At. Cl03-(aq) + 91. (aq)+ 6 H+ (aq) → 31.3 (aq) + Cl-(aq) + 3H20...