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Classify the half-reactions as reduction half-reactions or oxidation half-reactions. H(g)2 H (aq) +2e Answer Bank 0,...
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
(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...
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half reaction. identification half-reaction Ni (aq)+2e reduction Ni(s) Cd2 (aq) +2e oxidation Cd(s)- (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. + +
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Part III: Oxidation and Reduction of H2O2 1. Reduction of H2O2: H2O2(aq) + Cr(OH)3(S) (BASIC) • Observations · Evidence of the oxidation of Cr3+ • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction · Explain occurrence or non-occurrence of reaction by calculating cell. 2. Oxidation of H2O2: H2O2(aq) + FeCl3(aq) • Observations • Evidence of the oxidation of H2O2 • Reduction Half Reaction • Oxidation Half Reaction • Overall Balanced Redox Reaction • Explain occurrence or...
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. 2H+ + 2e - H2 Fe3+ + 3e + Fe Sn2+ + 2e Fe2+ + 2e →...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
Selective Reduction The standard reduction potential for the half-reaction: Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. no yes yes yes yes yes Fe — Fe2+ + 2e- Sn2+ Sn4+ + 2e- Sn Sn2+...
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Cd(s)Cd2+(aq) + 2e- Ag+(aq) + e-Ag(s) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. ? + ? ? + ? 2. Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Mn(s)Mn2+(aq) + 2e- Zn2+(aq) + 2e-Zn(s) (2) Write a balanced equation for the overall redox reaction. Use smallest...