Cars are powered by lead-acid batteries and the electrochemical cell processes are described the following net redox reaction: Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H₂O(1) Identify which ONE of the following statements is CORRECT? O a. Lead as both the metal and in the ionic compound is reduced and hydrogen is oxidised. O b. Lead as both the metal and in the ionic compound is oxidised and hydrogen is reduced. O c. Lead in the ionic compound is reduced and metallic lead is oxidised. d. Lead as both the metal and in the ionic compound is oxidised and oxygen is reduced. O e. Oxygen is oxidised and lead as both the metal and in the ionic compound is reduced.

Balance the following redox reaction.  For the said reaction, indicate the species that is oxidized and the one that is reduced, and identify the oxidizing and reducing agents. Cl2 (g)               è         Cl- (aq)     +     OCl- (aq)                                     (basic)

Give detailed Solution

Which is the balanced chemical equation for the following redox reaction in a basic medium?   MnO4- + SO32- → MnO2 + SO42-   2MnO4- + 3SO32- + H2O → 2MnO2 + 3SO42- + 2OH-   MnO4- + SO32- → MnO2 + SO42-   MnO4- + SO32- + 2H+ → MnO2 + SO42- + H2O   2MnO4- + 3SO32- + 2H+ → 2MnO2 + 3SO42- + H2O   Given the reaction of the synthesis of ethyl acetate:   CH3COCH3 + Br2 + H3O+ → CH3COCH2Br + HBr + H3O+ Which is the catalyst?   H3O+    CH3COCH3   CH3COCH2Br   Br2   3. Calculate the order of reaction with respect to O2.   1.5   2   1   0

4. Cu(s) + 2 AgNO,(aq) → Circle one: VOLTAIC / ELECTROLYTIC Substance oxidized: Substance reduced:

99. Consider the unbalanced redox reaction: MnO4¯¯ (aq) + Zn (s) → Mn²+ (aq) + Zn²+ (aq) Balance the equation and determine the volume of a 0.500 M KMnO4 solution required to completely react with 2.85 g of Zn.

/variants/1189727/take/9/ ☆ 88 MULTIPLE CHOICE Question 10 Which half-reaction correctly represents oxidation? Fe(s) → Fe +2 A Fe(s) B Fe +2 (aq) + 2e¯ (aq) → Fe(s) + 2e- + 2e → Fe+2 (ag) D Fe +2 (aq) + 2e¯ → Fe(s)

Balance the following redox reaction by adding the coefficients for each of the species.   Al(s)+F2(g)→Al3+(aq)+F−(aq)   When I first answered this question I put a 2 in front of the F on the product side. After submitting my answer the program said that it was incorrect. Before sending in a question I found the problem on bartleby and it said that putting a 2 in front of the F on the product side would make my answer correct. What am I missing? Sorry about my first question, I meant to include the equation.

Specify whether the reactants of the given half-reaction is an oxidizing or reducing agent. VO, (aq) → V² (aq) AsH3(g) → As(s) Ag(s)→ Ag₂O(s) Cr(s) → Cr³+ (aq) (in acid) (in acid) (in base) (in acid) Choose... Choose... Choose... Choose... + + +

49. For each unbalanced equation given below write unbalanced half-reactions. • identify the species oxidized and the species reduced. identify the oxidizing and reducing agents. only no.50 to answer 50. Follow the directions of Question 49 for the following unbalanced equations. Ni³+(aq) + H2O (a) H2O2(aq) + Ni²+(aq) - (b) Cr,O;²-(aq) + Sn²+(aq) - Cr³*(aq) + Sn++(aq)