1. What occurs during the operation of a voltaic cell based on the following reaction? Ni (s) +Pb2+(aq) > Ni2+(aq) +Pb(s) External circuitIon movement in solution A. electrons move from Ni to PbPb2+(aq) move away from Pb(s) B. electrons move from Ni to PbPb2+(aq) move toward Pb(s) C. electrons move from Pb to NiNi2+(aq) move away from Ni(s) D. electrons move from Pb to NiNi2+(aq) move toward Ni(s) (2) 2. Which processes occur during the electrolysis of molten sodium chloride? I. Sodium and chloride ions move through the electrolyte. II. Electrons move through the external circuit. III. Oxidation takes place at the positive electrode (anode).
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A. I and II only B. I and III only C. II and III only D. I, II and III (2) 3. What happens to the Cr3+(aq) ion when it is converted to CrO (aq)? A. Its oxidation number decreases and it undergoes reduction. B. Its oxidation number decreases and it undergoes oxidation. C. Its oxidation number increases and it undergoes reduction. D. Its oxidation number increases and it undergoes oxidation. (2) ? 4. The following reactions are spontaneous as written. Fe(s) + Cd2+(aq) > Fe2+(aq) + Cd(s) Cd(s) + Sn2+(aq) > Cd2+(aq) + Sn(s) Sn(s) + Pb2+(aq) > Sn2+(aq) + Pb(s) Which of the following pairs will react spontaneously? I. Sn(s) + Fe2+(aq) II.
Cd(s) + Pb2+(aq) III. Fe(s) + Pb2+(aq) A. I only B. II only C. III only D. II and III only (2) 5. What species are produced at the positive and negative electrodes during the electrolysis of molten sodium chloride? Positive electrodeNegative electrode A. Na+(l)Cl2(g) B. Cl? (l)Na+(l) C. Na(l)Cl2(g) D. Cl2(g)Na(l) (2) 6. Consider the following reaction. H2SO3(aq) + Sn4+(aq) + H2O(l) > Sn2+(aq) + HSO (aq) + 3H+(aq) Which statement is correct? A. H2SO3 is the reducing agent because it undergoes reduction. B. H2SO3 is the reducing agent because it undergoes oxidation. C. Sn4+ is the oxidizing agent because it undergoes oxidation. D.
Sn4+ is the reducing agent because it undergoes oxidation. (2) 7. What happens at the positive electrode in a voltaic cell and in an electrolytic cell? Voltaic cellElectrolytic cell A. OxidationReduction B. ReductionOxidation C. OxidationOxidation D. ReductionReduction (2) 8. A voltaic cell is made from copper and zinc half-cells. The equation for the reaction occurring in the cell is Zn(s) + Cu2+(aq) > Zn2+(aq) + Cu(s) Which statement is correct when the cell produces electricity? A. Electrons are lost from zinc atoms. B. The mass of the copper electrode decreases. C. Electrons flow from the copper half-cell to the zinc half-cell. D.
Negative ions flow through the salt bridge from the zinc half-cell to the copper half-cell. (2) 9. What happens when molten sodium chloride is electrolysed in an electrolytic cell? A. Chlorine is produced at the positive electrode. B. Sodium ions lose electrons at the negative electrode. C. Electrons flow through the liquid from the negative electrode to the positive electrode. D. Oxidation occurs at the negative electrode and reduction at the positive electrode. (2) 10. Ag(s) + (aq) + H+(aq) ? Ag+(aq) + NO(g) + H2O(l) When the oxidation-reduction equation above is balanced, what is the coefficient for H+ (aq)?? A. 1 B. 2 C. 3 D. 4 (2)