
In the following reaction 2MnO4 (aq) + H2O(l) + 35032-lag) —>2MnOz(s) + 350,2-laq) + 2OH(aq) what...
Which is the anode in the following oxidation reduction reaction? 3NO2−(aq) + 2MnO4−(aq) +H2O(l) →3NO3−(aq) + 2MnO2(aq) +2OH−(aq) a) There is no anode in this reaction b) H2O(l) c) MnO4−(aq) d) NO2−(aq)
2MnO4−(aq)+3S2−(aq)+4H2O(l)→3S(s)+2MnO2(s)+8OH−(aq) elements changing the oxidation number are: 4H2O2(aq)+Cl2O7(g)+2OH−(aq)→2ClO2−(aq)+5H2O(l)+4O2(g) the elements changing oxidationn numbers are: Ba2+(aq)+2OH−(aq)+H2O2(aq)+2ClO2(aq)→Ba(ClO2)2(s)+2H2O(l)+O2(g) the elements changing oxidation are:
0.540 Eo cell = 0.956 4) Should the reaction, 2MnO2 (s) + 3CIO (aq) + 2OH; (aq) + 2MnO4 (aq) + 3Cl (aq) + H20 (1), occur spontaneously in the forward direction under standard-state conditions? Show your work. E cell so Spontaneus: Eccell - Eocell = Ered (Catrode) - Fored (anode) 0.956 - 0,340 = 0.616 Should the reaction, 2MnO2 (s) + 3CIO (aq) + 20H (aq) - 2MnO4 (aq) + 3Cl(aq) + H2O (1),occur spontaneously in the forward direction...
What are the Redox half reactions for this chemical equation? 2MnO2(s) + 3ClO-(aq) + 2OH-(aq) = 2MnO4-(aq) + 3Cl-(aq) + H2O(l)?
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq)2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq) Fe(s)⟶Fe2+(aq)+2e−Fe(s)⟶Fe2+(aq)+2e− oxidation reduction reduction oxidation reduction
Consider the reaction: Ba^2+ (aq) + 2OH^- (aq) → Ba(OH)2 (s) This reaction is NOT considered a redox reaction because: a) It only results in the formation of one product b) It only involves the oxidation of barium c) the oxidation number of the element does not change d) the product is in the solid state e) it only involves the reduction of barium
For the reaction 2ClO2(aq) + 2OH-(aq) --> ClO3-(aq) + H2O(l) the rate law is written Rate = k [ClO2]2 [OH-] a. What is the reaction order with respect to ClO2? _____________ b. Is the reaction order with respect to OH- second order? Why or why not? c. What is the overall reaction order? ____________________ d. If the concentration of ClO2 is doubled, the rate of the reaction would increase by a factor of ____________. Show how was the answer determined?
Write balanced half-reactions for the following redox reaction: 5I2(s)+2Mn^2+(aq)+16OH^-(aq)=10I^-(aq)+2MnO4^-(aq)+8H2O(l)
hvv C 1 of 15 Reduction Anode - Oxidation Cathode 2MnO4(s) + H2O()+22- - MnO,(s) +24,00 C Electron flow Carbon rod Membrane Zn(s) + 20H" (aq) → ZnO(s) +H,1) +2e" C El flaw 76% 3 0 0 0 0 2:07 PM 2020 O i
Question 6 (1 point) What is true about the following reaction at 25°C?<br /> LiBrO(aq) + H2O(l) = HBrO(aq) + LiOH(aq) O AGº > 0. The reactants are more stable than the products. OAG° > 0. The products are more stable than the reactants. O AG° < 0: The reactants are more stable than the products. O AG° < 0. The products are more stable than the reactants.