Which of the following statement/s is/are false?V All spontaneous oxidation-reduction reactions have an E°,cellwitha negative sign.O The anode of a battery is the site of reduction and is negative.O Standard conditions for electrochemical cells are a concentration of 1.0 M fordissolved species and 1.0 atm pressure for gases.Oxidation always occurs at the anode part of a spontaneous cell.The potential of the cell does not change with temperature.

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Answered: Which of the following statement/s…

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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Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) | Sn² + (0.0062 M). Sn +(0.15 M) || Fe +(0.11 M), Fe²+(0.0045 M) | Pt(s) ES' *Sn²+ = 0.154 V EF = 0.771 V Ecell 0.613 Incorrect Is the electrochemical cell spontaneous or not spontaneous as written at 25 "C? spontaneous not spontaneous
4
14. Calculate the equilibrium constant K, for the following balanced redox reaction at 25oC. (R = 8.31 J/mol.K). Pb2+(aq) + 2Ag(s) → Pb(s) + Ag+(aq) given the following standard redox potentials: Pb2+(aq) + 2e- ⟶⟶ Pb(s) E0 = -0.13 V Ag+(aq) + e-⟶⟶ Ag(s) E0 = 0.80 V A. 72.47 B. 3 x 1031 C. 0.93 D. 4.9 x 1011 E. 3 x 10-32
Chemistry 19.10.-Calculate the standard potential, ,E°, for this reaction from its AG° value. X(s)+Y4+(aq)-X4+(aq)+Y(s) AG•=31.0 kJ
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
A redox reaction used in an electrochemical cell has a negative standard free energy change, AGxn- Which statement about the redox reaction is true? O Ecel is positive; K 1 E'cel is negative; K 1 'cell
nge in 5 on 6 O tion 7 stion 8 estion 9 " Question 10 11 Submit Use the References to access important values if needed for this question. A Fe Fe²+ || Cd²+ | Cd galvanic cell is constructed in which the standard cell voltage is 3.70×10:2 V. Calculate the free energy change at 25°C when 0.863 g of Cd plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? Submit Answer 5 question attempts remaining AGⓇ Maximum work= X A
The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) → 2 H₂O(l) K = 1.34 x 1083 (a) Calculate and AG at 298 K for the fuel-cell reaction. V k] 80 AGO (b) Predict the signs of AH° and AS for the fuel-cell reaction. AH°: O positive. O negative AS°: positive O negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. Since AS is ---Select---, as T increases, AG becomes more ---Select--- . Therefore, the maximum work obtained will ---Select--- as T increases. ASK YOUR TEACH
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
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