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BALANCING REDOX REACTIONS
Use the half-reaction method to balance each
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Introductory Chemistry, Books a la Carte Edition (5th Edition)
- Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).arrow_forwardWhich of the following elements is the best reducing agent under standard conditions? (a) Cu (b) Zn (c) Fe (d) Ag (e) Crarrow_forwardBalance the following skeleton equations. The reactions occur in acidic or basic aqueous solution, as indicated. a MnO4+S2MnO2+S8(basic) b IO3+HSO3I+SO42(acidic) c Fe(OH)2+CrO42Fe(OH)3+Ce(OH)4(basic) d Cl2Cl+ClO(basic)arrow_forward
- An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. If the copper electrode is placed in a solution of 0.10 M NaOH that is saturated with Cu(OH)2, what is the cell potential at 25C? [For Cu(OH)2, Ksp = 1.6 1019.]arrow_forwardUse electrode potentials to answer the following questions, assuming standard conditions. a Do you expect permanganate ion (MnO4 ) to oxidize chloride ion to chlorine gas in acidic solution? b Will dichromate ion (Cr2O72) oxidize chloride ion to chlorine gas in acidic solution?arrow_forwardAn electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forward
- What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?arrow_forwardCadmium sulfide is used in some semiconductor applications. Calculate the value of the solubility product constant (Ksp) for CdS given (he following standard reduction potentials: Cds(s) + 2e Cd(s) + s2(aq) = 1.21 V Cd2+ (aq) + 2e Cd(s) = 0.402 Varrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forward
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