The free energy change for the following reaction at 25 °C, when [H]= 3.34×103 M and [Hg**]= 1.15 M, is 180. kJ: 2H*(3.34×103 M) – Hg() H2(g) - Hg*1.15 M) AG = 180. kJ What is the cell potential for the reaction as written under these conditions? Answer: -0.932 |v Would this reaction be spontaneous in the forward or the reverse direction? forward v

The free energy change for the following reaction at 25 °C, when [H]= 3.34×103 M and [Hg**]= 1.15 M, is 180. kJ: 2H(3.34×103 M) – Hg() H2(g) - Hg1.15 M) AG = 180. kJ What is the cell potential for the reaction as written under these conditions? Answer: -0.932 |v Would this reaction be spontaneous in the forward or the reverse direction? forward 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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6. Consider the following cell: Zn(s)|ZnCl,(0.005 mol kg')|Hg,Cl(s)|Hg() The cell reaction is Hg,Cl2(s)+Zn(s) →2Hg(1)+2Cl'(aq)+Zn**(aq) E (Zn*, Zn)=-0.7628 V E (Hg,Cl,, Hg)=+0.2676 V Calculate the electromotive force of this cell at 25 °C., neglecting the correction of activity coefficient. а. b. Assuming that the Debye-Hückel limiting law holds at this concentration, calculate the electromotive force again. с. Calculate AG of this cell, using the electromotive force from part b.
[References) What are the reaction quotient (Q) and the calculated value of the cell potential (Ecell) at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 7.35x104 M and the Mg²* concentration is 1.25 M? Hg"(aq) + Mg(s) Hg(l) + Mg²+(aq) E°cell = 3.225 V Q= Ecel =|
Use the standard half-cell potentials Click to open: to calculate the standard cell potential (Eºcell) and the standard free energy (AGO) for the following reaction. • Answer: Eºcell = [Select] . Answer: AG° = [Select] Co(s) + F2(g) → Co2+ (aq) + 2F (aq) V kJ
The free energy change for the following reaction at 25 °C, when [Ag*] = 1.20 M and [Cu2+] = 8.38x10-3 M, is -101 kJ: 2Ag*(1.20 M) + Cu(s)2Ag(s) + Cu2+(8.38x10-3 M) AG = -101 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse
What is the correct shorthand notation for the cell on the previous slide? Oxidation: Ag(s) Ag*(aq) + e- Reduction: Mno,(s) + 4 H*(ag) + 2 e - Mn2+(aq) + 2 H,0() A. Ag(s) | Ag*(aq) || H*(aq), Mn²*(aq), H20() | MnOg(s) В. Ag*(aq) | Ag(e) || Mn02(a) | Mn²*(aq), H20(). H*(aq) C. Mno2(3) | H*(aq), Mn²*(aq), H20() || Ag*(aq) | Ag(3) D. Mn2*(aq). H20(). H*(@q) | MnO2(s) || Ag(3) | Ag*(aq)
(Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction that occurs in an electrochemical cell at 25°C? Fe3+ (aq) + Cu* (aq) ---> Fe²+ (aq) + Cu2+ (aq) The reduction potentials for the two half-reactions involved are: Fe3+ + e- --> Fe2+ (E°RED) = 0.77 V Cu2+ + e- --> Cu* (E°RED) = 0.16 V %3D
Item 1 < 1 of 25 Constants | Periodic Table Part A The standard cell potential (E') of the reaction below is -0.55 V. The value of A G for the reaction is J/mol. I2 (5) + 2Br (aq) → 21 (aq) + Brz (1) O 1.1- 105 O 0.54 O 0.55 O 5.5 - 106 O none of the above Submit Request Answer
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Sn²+] = 0.00140 M and [Au³+] = 0.841 M. Standard reduction potentials can be found in this table. 3 Sn(s) + 2 Au³+(aq) = 3 Sn²+(aq) + 2 Au(s) E = V * TOOLS x10
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Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.879 M and [Sn²+] = 0.0190 M. Use the standard reduction potentials in this table. Zn(s) + Sn²+ (aq) = Zn²+ (aq) + Sn(s) V I Enter numeric value TOOLS E = x10 MacBook Air
3) Use half cell potentials to determine if each reaction occur spontaneous in the direction written (yes/no). a) Ca¹2(aq) + Zn(s) - Ca(s) + Zn¹²(aq) b) Au*³(aq) + Ag(s) - Au(s) + Ag (aq) c) Co(s) + Pb (aq) - Co²(aq) + Pb(s) d) Pb(aq) + H₂S(g) -Pb¹2(aq) + S(s) ing if each metal will dissolve in 1M HCl.