Consider R2* at standard conditions. What is the E°cell (in volts)? Final answer: two decimal places; include negative sign whenever applicable; no unit necessary. Use data given inTable 1.2R3+(aq) + 2J'(aq) – 2R2*(aq) + J2(s) hypothetical reactionTable 1. Standard Reduction Potentials at 25°C of Some Hypothetical SubstancesA3+ + 3e - AE° = + 1.4 Vx2+ + 2e -XEO = - 2.87 VR3+ + e - R2+E° = + 0.67 VJ2 + 2e - 2JE° = + 0.27 V12+ + 2e -LE° = - 2.36 VT2+ + 2e -TE° = -0.14 V

At anode : oxidation 2J- (aq) ----> J2 (s) + 2e- E° (j2 / j-) = + 0.27 V -- equation (1)…

Consider R2* at standard conditions. What is the E°cell (in volts)? Final answer: two decimal places; include negative sign whenever applicable; no unit necessary. Use data given in Table 1. 2R3*(ag) + 2J"(aq) – 2R2*(aq) + J2(s) hypothetical reaction Table 1. Standard Reduction Potentials at 25°c of Some Hypothetical Substances A3+ + 3e -A E° = + 1.4 V x2+ + 2e -X E° = - 2.87 V R3+ + e - R2+ E° = + 0.67 V J2 + 2e - 2J E° = + 0.27 V 12+ + 2e -L E° = - 2.36 V T2* + 2e -T E° = -0.14 V

Consider R2* at standard conditions. What is the E°cell (in volts)? Final answer: two decimal places; include negative sign whenever applicable; no unit necessary. Use data given in Table 1. 2R3(ag) + 2J"(aq) – 2R2(aq) + J2(s) hypothetical reaction Table 1. Standard Reduction Potentials at 25°c of Some Hypothetical Substances A3+ + 3e -A E° = + 1.4 V x2+ + 2e -X E° = - 2.87 V R3+ + e - R2+ E° = + 0.67 V J2 + 2e - 2J E° = + 0.27 V 12+ + 2e -L E° = - 2.36 V T2* + 2e -T E° = -0.14 V

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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heres the link for the data table http://chemistry-reference.com/tables/Table%20of%20Standard%20Reduction%20Potentials%20and%20Activity%20Series.pdf
heres the link to the data table http://chemistry-reference.com/tables/Table%20of%20Standard%20Reduction%20Potentials%20and%20Activity%20Series.pdf
Consider the following reaction and standard reduction potential data. 2Ag (aq) + Cu(s) 2Ag(s) + Cu*"(aq) Half reaction E°(V) Ag (aq) +eAg(s) 0.80 Cu2"(aq) + 2e → Cu(s) 0.34 a. As written, is the Keg of the reaction shown above greater than 1 or less than 17 (Select] b. Which species is the reducing agent? [Select ] c. Suppose a voltaic cell was constructed using a Cu and Ag electrode (pictured below). The Cu electrode was placed in a 0.01 M solution of Cu(NO;)2, and the Ag electrode was placed in a 1.00 M solution of AGNO3. What is the Ecell for this voltaic cell? Assume the temperature is 298 K. Also NO; is a spectator ion. ( Select ) Voltmeter Ag Cu sat bridge AgNO= 1.00 M -0.01 M >
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Mm.45.
What mass of Fe(s) may be deposited from an aqueous FeCl2 solution if a current of 2.50 A is applied to the solution for 365 s? (ε°red(Fe2+/Fe) = -0.447 V, F = 96485 C/mol)
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Oo.98. Subject :- Chemistry