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Here's an example: Balance the following redox reaction, which occurs...
When the following reaction is balanced under basic conditions, what is the ratio of the coefficients...
When the following reaction is balanced under basic conditions, what is the ratio of the coefficients of Mn(OH)2(s) to MnO4--(aq)? Mn(OH)2(s) + MnO4 (aq) + MnO42-(aq) (A) 3:1 (B) 1:3 (C) 1:4 (D) 1:5 What is the standard reduction potential for the reduction of permanganate ion to managanese dioxide in acidic solution? Half-Reaction E. V MnO4 (aq) + 8 H(aq) + 5 € → Mn²+ (aq) + +1.51 4 H2O(1) MnO2(s) + 4 H (aq) + 2 e → Mn2+(aq)...
Balance Redox Equations (Acidic Solutions) show steps please. 1. HgS (s) + NO3^- (aq) + Cl^-...
Balance Redox Equations (Acidic Solutions) show steps please. 1. HgS (s) + NO3^- (aq) + Cl^- (aq) = HgCl4^2- (aq) + NO (g) + S (s) 2. Fe^2+ (aq) + MnO4^- (aq) = Fe^3+ (aq) + Mn^2+ (aq) 3. BiO3^- (aq) + Mn^2+ (aq) = MnO4^- (aq) + Bi^3 (aq) 4. NiO2 (s) + Ag (s) = Ni^2+ (aq) + Ag^+ (aq) 5. IO3^- (aq) + I^- (aq) =I2 (s) 6. Zn (s) + H2SO4 (aq) = Zn^2+ (aq) +...
please answer in 10m 5. Balance each reaction, calculate the net Eº, and declare each reaction...
please answer in 10m
5. Balance each reaction, calculate the net Eº, and declare each reaction as being spontaneous or non- spontaneous. (9) a) Sn?' (aq) + Cr(s) → Sn(s) + Cr?" (aq) net Eº = b) Ag+ (aq) + Mn(s) Ag(s) + Mn2(aq) net Eº = c) Fe2(aq) + Cu(s) → Fe(s) + Cu?"(aq) net Eº =
Step 1: Determine whether or not each redox reaction occurs spontaneously in the forward direction using...
Step 1: Determine whether or not each redox reaction occurs
spontaneously in the forward direction using only the relative
postion of the half reactions on table 18.1. (No numbers in this
step.)
Step 2: Then, calculate the voltage of each of the
reactions.
(a) Ca2+(aq) + Zn(s)
Ca(s) + Zn2+(aq)
(b) 2Ag+(aq) + Ni(s)
2Ag(s) + Ni2+(aq)
(c) Fe(s) + Mn2+
Fe2+(aq) Mn(s)
Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0,...
Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equatio 1-SO3-(ag)+MnO4-(ag)+H+(ag)---->SO4^2-(ag)+Mn2+(ag)+H2O(l) 2- H2O2(ag)+ClO2(ag)+HO-(ag)---> O2(g)+ClO2-(ag)+H2O(l) Q: In the electrochemical voltaic cell using the reaction, Fe3+(aq) + Cr(s) → Fe(s) + Cr3+(aq), match the correct 1/2 reaction that occurs at the anode and cathode. 1/2 reaction occuring at the anode 1/2 Reaction occuring at the cathode Choices: A Fe3+(aq) +...
19. a. Balance the following redox reaction if it occurs in acidic solution. How many electrons...
19. a. Balance the following redox reaction if it occurs in acidic solution. How many electrons are transferred, and what are the half reaction potentials? Fe 2+(aq) + MnO4 ?(aq) ? Fe 3+(aq) + Mn 2+(aq) b. What element is being oxidized, and what is the oxidizing agent in the given redox reaction? Mg2+(aq) + NH4 +(aq) ? Mg(s) + NO3 ?(aq)
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a....
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
Need help with questions 1-5 D Determine whether each redox reaction occurs spontane- ously in the...
Need help with questions 1-5
D Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca2+(aq) + Zn(s)-Ca(s) + Zr"(al) (b) 2 Ag+(aq) + Ni(s)--2 Ag(s) + N产(aq) (c) Fe(s) +Mn2 (aą)- Fe (aą)Mn(s) (d) 2 Al(s) + 3 Pb2+(aq) → 2 AP"(aq) + 3 Pb(s) Suppose you wanted to cause Pb ions to come out of solu- tion as solid Pb. What metal could you use to accomplish this? Make a sketch of an electrochemical...
Balance the following Redox reaction, which occurs in Acidic solution: Mn2+ (aq) MnO4 (aq) + H,C204(aq)...
Balance the following Redox reaction, which occurs in Acidic solution: Mn2+ (aq) MnO4 (aq) + H,C204(aq) + CO2(aq)
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
When the following reaction is balanced under basic conditions, what is the ratio of the coefficients of Mn(OH)2(s) to MnO4--(aq)? Mn(OH)2(s) + MnO4 (aq) + MnO42-(aq) (A) 3:1 (B) 1:3 (C) 1:4 (D) 1:5 What is the standard reduction potential for the reduction of permanganate ion to managanese dioxide in acidic solution? Half-Reaction E. V MnO4 (aq) + 8 H(aq) + 5 € → Mn²+ (aq) + +1.51 4 H2O(1) MnO2(s) + 4 H (aq) + 2 e → Mn2+(aq)...
please answer in 10m
5. Balance each reaction, calculate the net Eº, and declare each reaction as being spontaneous or non- spontaneous. (9) a) Sn?' (aq) + Cr(s) → Sn(s) + Cr?" (aq) net Eº = b) Ag+ (aq) + Mn(s) Ag(s) + Mn2(aq) net Eº = c) Fe2(aq) + Cu(s) → Fe(s) + Cu?"(aq) net Eº =
Step 1: Determine whether or not each redox reaction occurs
spontaneously in the forward direction using only the relative
postion of the half reactions on table 18.1. (No numbers in this
step.)
Step 2: Then, calculate the voltage of each of the
reactions.
(a) Ca2+(aq) + Zn(s)
Ca(s) + Zn2+(aq)
(b) 2Ag+(aq) + Ni(s)
2Ag(s) + Ni2+(aq)
(c) Fe(s) + Mn2+
Fe2+(aq) Mn(s)
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
Need help with questions 1-5
D Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca2+(aq) + Zn(s)-Ca(s) + Zr"(al) (b) 2 Ag+(aq) + Ni(s)--2 Ag(s) + N产(aq) (c) Fe(s) +Mn2 (aą)- Fe (aą)Mn(s) (d) 2 Al(s) + 3 Pb2+(aq) → 2 AP"(aq) + 3 Pb(s) Suppose you wanted to cause Pb ions to come out of solu- tion as solid Pb. What metal could you use to accomplish this? Make a sketch of an electrochemical...
Balance the following Redox reaction, which occurs in Acidic solution: Mn2+ (aq) MnO4 (aq) + H,C204(aq) + CO2(aq)
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
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