Question

In: Chemistry

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M) + H2(1 atm) ?...

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M) + H2(1 atm) ? 2Ag(s) + 2H+(pH = 8.00)

Solutions

Expert Solution

First, some tabulated data:
Ag+ (aq) + e− ==> Ag(s), Eº = 0.80
2 H+ (aq) + 2 e− ==> H2(g), Eº = 0.00

Since your cell isn't in standard (all solutions 1 M, all gases 1 atm), you must use Nernst's equation to account for this difference. It states that:
E = Eº - (RT/nF) ln([Red]/[Ox]),
where R and F are the ideal gas' and Faraday's, constants respectively, n the ammount of electrons involved and [Red] and [Ox] the concentrations of the oxidated and reduced compounds involved, respectively. Since no temperature is stated, we'll supose the standard 25ºC, and rewrite the equation as:
E = Eº - (0.0591/n) log([Red]/[Ox]).
Solids and the solvent have an activity of 1, and thus can be left out of this equation. In the case of gases, their partial pressure is used instead of their concentration.

So, for the silver's half-reaction:
Ag+ (aq) + e− ==> Ag(s), Eº = 0.80
And E = Eº - (0.0591/n) log([Red]/[Ox]) becomes:
E = 0.80 - (0.0591/1) log(1/[Ag+])
E = 0.80 + 0.0591 log([Ag+])
For [Ag+] = 0.010 M,
E = 0.80 + 0.0591 log(0.010)
E = 0.80 - 2*0.0591
E = 0.6818

And for hydrogen's:
2 H+ (aq) + 2 e− ==> H2(g), Eº = 0.00
And E = Eº - (0.0591/n) log([Red]/[Ox]) becomes:
E = - (0.0591/2) log((H2)/[H+]^2)
E = - 0.02955 log((H2)/[H+]^2)
E = - 0.02955 log((H2)) + 0.0591 log([H+])
E = - 0.02955 log((H2)) - 0.0591 pH
For (H2) = 1 atm and pH = 8.0,
E = - 0.02955 log(1) - 0.0591*8.0
E = - 0.4728

So, the cell's E is:
Ecell = Ered - Eox
Ecell = 0.6818 + 0.4728
Ecell = 1.1546 V


Related Solutions

What is the emf of a cell consisting of a Pb2+ / Pb half-cell and a Pt / H+ / H2 half-cell if [Pb2+] = 0.46 M, [H+] = 0.047 M and PH2 = 1.0 atm ?
What is the emf of a cell consisting of a Pb2+ / Pb half-cell and a Pt / H+ / H2 half-cell if [Pb2+] = 0.46 M, [H+] = 0.047 M and PH2 = 1.0 atm ?____V
Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If...
Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.236 volts, what is the pH of the hydrogen electrode? A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.202 V, what is the pH of the unknown solution at 298...
Calculate the [H+] and [OH-] of each of the following solutions. 0.010 M HCl 0.010 M...
Calculate the [H+] and [OH-] of each of the following solutions. 0.010 M HCl 0.010 M H2SeO4 0.025 M KOH 0.020 M Ba(OH)2
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Ni(s)+2Ag+(aq)→Ni2+(aq)+2Ag(s), if Ni2+(aq)+2e−→Ni(s), E∘...
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Ni(s)+2Ag+(aq)→Ni2+(aq)+2Ag(s), if Ni2+(aq)+2e−→Ni(s), E∘ = -0.26 V, Al+(aq)+e−→Al(s), E∘ = 0.80 V Express your answer using one significant figure. Part B Calculate the equilibrium constant at 25 ∘C for the reaction Hg2+2(aq)→Hg(l)+Hg2+(aq) See Appendix D for standard reduction potentials. Express your answer using one significant figure.
Calculate the EMF of the cell: Al(s) | Al3+ (0.02 M) || Au+ (0.01 M) |...
Calculate the EMF of the cell: Al(s) | Al3+ (0.02 M) || Au+ (0.01 M) | Au(s) Where Al3+ + 3e-  Al E o= -1.66 V Where Au+ + e-  Au E o = +0.99 V
Calculate the cell potential for the galvanic cell in which the following reaction occurs at 25...
Calculate the cell potential for the galvanic cell in which the following reaction occurs at 25 °C, given that [Al3 ] = 0.00120 M and [Au3 ] = 0.787 M. Al (s) + Au^3+ (aq) <===> Al^3+ (aq) + Au (s)
At 1 atm and 25 ˚C the molar entropy change for the reaction CO(g) + 1...
At 1 atm and 25 ˚C the molar entropy change for the reaction CO(g) + 1 2 O2(g)  CO2(g) (1) is ΔSo = - 86.46 J K-1. The molar heat capacities at constant pressure at 1 atm and 25 ˚C for CO, O2, and CO2 are, respectively, 29.123, 29.362, and 37.12 J K-1 mol-1. Assume that the heat capacities are independent of temperature and calculate the entropy change for reaction (1) at 100 ˚C and 1 atm.
Calculate ΔGº at 25ºC for the reaction H2 + I2 D 2HI. Starting with 1.0 atm...
Calculate ΔGº at 25ºC for the reaction H2 + I2 D 2HI. Starting with 1.0 atm H2 and 1.0 atm I2, What is ΔG when: 0.1%, 1%, 10%, 50%, 90%, 99%, and 99.9% has reacted.
Calculate ΔGo at 25oC for the reaction H2 + I2 D 2HI. Starting with 1.0 atm...
Calculate ΔGo at 25oC for the reaction H2 + I2 D 2HI. Starting with 1.0 atm H2 and 1.0 atm I2, What is ΔG when: 0.1%, 1%, 10%, 50%, 90%, 99%, and 99.9% has reacted.
Calculate the standard enthalpy change for the following reaction at 25 °C. H2O(g)+C(graphite)(s) ----> H2(g)+CO(g) deltaH...
Calculate the standard enthalpy change for the following reaction at 25 °C. H2O(g)+C(graphite)(s) ----> H2(g)+CO(g) deltaH rxn=_____kJ
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT