(a)
Interpretation:
The given
Concept introduction:
The oxidizer is the species whose oxidation state decreases during the course of reaction and reducer is the species whose oxidation number increases. Oxidized product is the oxidation product of the reducer and reduced product is the reduction product of the oxidizer.
(b)
Interpretation:
The given redox reaction is spontaneous or nonspontaneous is to be stated.
Concept introduction:
The oxidizer is the species whose oxidation state decreases during the course of reaction and reducer is the species whose oxidation number increases. Oxidized product is the oxidation product of the reducer and reduced product is the reduction product of the oxidizer.
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Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).arrow_forwardCalculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.arrow_forwardFor the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?arrow_forward
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- Calculate G at 355 K for each of the reactions in Question 17. State whether the reactions are spontaneous.arrow_forwardSome metals, such as thallium, can be oxidized to more than one oxidation state. Obtain the balanced net ionic equations for the following oxidation reduction reactions, in which nitric acid is reduced to nitric oxide, NO. a Oxidation of thallium metal to thallium(I) ion by nitric acid. b Oxidation of thallium(I) ion to thallium(III) ion by nitric acid. c Oxidation of thallium metal to thallium(III) by nitric acid. [Consider adding the a and b equations.]arrow_forward
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