Answer:-
The half reactions for the given balanced redox reaction are written using oxidation and reduction concept.
The answer is given in the image,
What are the Redox half reactions for this chemical equation? 2MnO2(s) + 3ClO-(aq) + 2OH-(aq) =...
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...
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:
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
Write balanced half-reactions for the following redox reaction: 5I2(s)+2Mn^2+(aq)+16OH^-(aq)=10I^-(aq)+2MnO4^-(aq)+8H2O(l)
REDOX REACTION In the following balanced redox equation, what mass of solid MnO2 is produced when 55 mL of 0.35 M NaI solution is mixed with 4.5 grams of KMnO4 dissolved in 250 mL of water? 6I-(aq) + 4H2O(l) + 2MnO4-(aq) → 3I2(aq) + 2MnO2(s) + 8OH-(aq)
What is this balanced equation? MnO4−(aq) + I−(aq) I2(s) + MnO2(s) I got 2MnO4-(aq) + 6I-(aq) + 4H2O(l) ⇌ 3I2(s) + 2MnO2(s) + 8OH-(aq) but webassign is saying it's wrong. edit: nevermind, figured it out. 2 MnO4-(aq) + 8 H+(aq) + 6I-(aq) ⇌ 3 I2(s) + 2 MnO2(s) + 4 H2O(l) Calculate values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole...
In the following reaction 2MnO4 (aq) + H2O(l) + 35032-lag) —>2MnOz(s) + 350,2-laq) + 2OH(aq) what is the change in oxidation number for S? 0 -3 O 0 +2 O-2 +3
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)
Which of the reactions involving metal ions (Equations 1A – 6B ) represent redox reaction(s)? Write down the entire equation(s) AS WELL AS their corresponding balanced oxidation half-reaction(s) AND reduction half-reaction(s). Ag+(aq)+ HCl(aq)+ H2O(l) -> AgCl(s, white)+ H3O+(aq) Eq. 1A AgCl(s)+ 2NH3(aq) -> [Ag(NH3)2]+(aq)+ Cl–(aq) Eq. 2A Fe3+(aq)+ 3NH3(aq)+ 3H2O(l) -> Fe(OH)3(s)+ 3NH4(aq) Eq. 3A Fe3+(aq)+ 6SCN–(aq) -> Fe(SCN)63–(aq, blood-red) Eq. 4A Co2+(aq)+ 7NO2–(aq)+ 3K+(aq)+ 2H3O+(aq) -> NO(g)+ 3H2O(l)+ K3[Co(NO2)6](s, yellow) Eq. 6A 2 NO(g, colorless)+ O2(g) →2NO2(g, red-brown) Eq....
Balance the following redox reactions by balancing the half reactions and then combine the half reactions to get the overall balanced redox reaction with the lowest possible whole number coefficients. 1. Consider the following unbalanced redox reaction: MnO2(s) + BrO3−(aq) → MnO4−(aq) + Br−(aq) (a) Balance the corresponding half reactions in acidic conditions using the lowest possible whole number coefficients. (Enter coefficients for one and zero. Blanks will be marked incorrect.) MnO2(s) + H2O(l) + OH−(aq) + H+(aq) + e− → MnO4−(aq) + H2O(l) + OH−(aq) + H+(aq)...