The standard reduction potential at 25°C of thereaction 2H2O + 2e¯¯ = H₂ + 20H is -0.84 V.Calculate equilibrium constant for the reaction:2H2O H3O++ OH at 25°C. (2.303 RT/F=0.06)(a) 10-14(c) 107(b) 1014(d) 107

We know reduction occurs at cathode and oxidation occurs at anodeGivencathode: H2O+e−→21H2+OH−…

Answered: The standard reduction potential at…

Chemistry

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 88E: For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1,...

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
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The standard reduction potential at 25°C of the reaction 2H2O + 2e¯¯ = H₂ + 20H is -0.84 V. Calculate equilibrium constant for the reaction: 2H2O H3O++ OH at 25°C. (2.303 RT/F=0.06) (a) 10-14 (c) 107 (b) 1014 (d) 107