1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO3- (aq)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3 – (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1.a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2 (g) → NO3– (aq) (ii) (acid solution) H2SeO3 (aq) → Se (s) (iii) (base solution) P4 (s) → PH3 (g) (iv) (base solution) Co(OH)3 (s) → CoO2 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) BiO;- (aq) → BIO+ (aq) (ii) (acid solution) C002 (s) → Co2+ (aq) (iii) (base solution) Cr(OH).- (aq) → CrO2- (aq) (iv) (base solution) TeO 2- (aq) → H.Te0.2- (aq) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
(a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) Cl– (aq) → ClO3– (aq) (ii) (acid solution) MoO3 (s) → Mo (s) (iii) (base solution) P4 (s) → H2PO2– (aq) (iv) (base solution) Se (s) → SeO32– (aq) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq) → SO42- (aq) (ii) (acid solution) Pu(OH)4 (8) ► Pu+ (aq) (iii) (base solution) CN- (aq) → OCN- (aq) (iv) (base solution) RhO42- (aq) → Rh,03 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reactic Balance the following redox equations by the ion-electron half-reaction method: (a) (acid...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) NO2(g) → NO,- (aq) (ii) (acid solution) H SeO(aq) → Se (s) (iii) (base solution) P (8) PH, (g) (iv) (base solution) Co(OH)(s) C002 () (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reaction.
(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...
3. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): Cr0(aq) + U" (aq) → Cr" (aq) +UO; (aq) (b) (acid solution): Cr(s) + O2(g) → Cr* (aq) (C) (basic solution): P. (s) + OH' (aq) → PH; (g) + H2PO2 (aq)
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...
Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO2 (s) + Cl → Mn2+ + Cl2 (g) (b) (acid solution): NaBiO; (s) + Ce3+ BiO+ + Ce4+ + Na+ (c) (basic solution): Fe(OH)2 (s) + CrO42- → Fe,0, (s) + Cr(OH)4