Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Fe²+(aq) + 2Fe²+(aq)→→→→→→Fe(s) + 2Fe³+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: Check & Submit Answer Show Approach

Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Fe²+(aq) + 2Fe²+(aq)→→→→→→Fe(s) + 2Fe³+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: Check & Submit Answer Show Approach

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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EHide blocks Stane #7 Calculate the standard potential for the reaction shown below at 25°? 6 Hg*2 (aq) + 2 MnO2 (s) + 8 OH (aq) 3 Hg2*2 (aq) + 2 MnO4 (aq) + 4 H2O (I) E° = %3D Check Next p NEXT ACTIVITY S ACTIVITY Writing Equations (PRACTICE ASSIGNMENT) - Not Required Jump to...
Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25 °C and standard conditions of 1 M for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E 2.303 RT 1 nF -log10 Q where E is the potential in volts. Eo is the standard potential at 25°C in volts. R 8.314 J/(K-mol) is the gas constant, T is the temperature in kelvins. 12 is the number of moles of electrons transferred, F = 96, 500 C/(mol e-) is the Faraday constant, and is the reaction quotient. At the common reference temperture of 298 K. substituting each constant into the equation the result is E = E- Vlog 10 Q 0.0592 V 71
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+ Cell Potential and Equilibrium The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K FE RT where 72 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▾ Part A Use the table Express your answer numerically. ▸ View Available Hint(s) K= ΥΠΙ ΑΣΦ 9 Reduction half-reaction Ag+ (aq) +eAg(s) Cu²+ (aq) +201 >Cu(s) Sn+ (aq) + 4e →→Sn(s) 2H+ (aq) +2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe²+ (aq) + 2e →Fe(s) Zn²+ (aq) +2e →Zn(s) Al³+ (aq) + 3e →Al(s) Mg²+ (aq) + 2e →Mg(s) standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s) ? E (V) 0.80 0.34 0.15 0 0.26 -0.45 0.76 -1.66 2.37 29 o Review | Constants | Period
▾ Part A For the reaction 2Co³+ (aq) + 2Cl(aq)-2Co2+ (aq) + Cl₂(g). E = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] = 0.495 M. [Co²+] = 0.295 M, and [CI] = 0.272 M, and the pressure of Cl₂ is Pc, = 8.50 atm ? Express your answer with the appropriate units. View Available Hint(s) E= Submit 0 HA Value Units GAEC LIST onstans Periodic Table ?
Given the cell: Zn | Zn²+ (0.100 M) || Co²+ (0.050 M) | Co Answer the ff. 1. The standard cell potential, Ecell is [Select] 2. The cell potential, Ecell is [Select] 3. The reaction is [Select] 23 Quiz saved at 6:44am N Su