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- Calculate the equilibrium constant for the redox reactions that could occur in the following situations and use that value to explain whether or not any reaction will be observed. (a) A piece of iron is placed in a 1.0 M solution of NiCl2(aq). (b) A copper wire is placed in a 1.0 M solution of Pb(NO3)2(aq).arrow_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: Ag+(aq); Cd2+(aq); MnO4(aq) (in acidic solution).arrow_forwardWhich of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.arrow_forward
- Consider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.arrow_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).arrow_forwardUse Table 17.1 to arrange the following oxidizing agents in order of increasing strength: Mn2+ S Co3+ Cl2 K+arrow_forward
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