For the reaction 2Co3+(aq)+2Cl(aq)->2Co2+(aq)+Cl2(g). Excell=0.46 V what is the cell potential at 25 °C if theconcentrations are [Co3+]=0.168mol L-1, [Co2+]=0.574mol L-1, and [CI-]=2.30\times 10-2mol L-1 and the pressure ofCl2 is PC12=9.70bar ?

Answer:Value of cell potential at 298.15K temperature is:Here:n is equal to number of electrons…

Answered: For the reaction…

Chemistry

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Chapter1: Chemical Foundations

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Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that 'Ce'[Sn'2] - 0.0652-text M[Sn²+] = 0.0652 M, 'Ce'[Co'3] - 0.0409-text M[Co³+] = 0.0409 M, 'Ce'[Sn'4] - 0.00496 'text' [Sn+] = 0.00496 M, and "C.[Co'2] - 0.01150 'text'[Co²+] = 0.01150 M. Standard reduction potentials can be found in this table. Sn²+(so much) + 2 Co³* (so much) = Sn* "(so much) + 2C0²+ (so much) E = V
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
Calculate the cell potential at 25oC for the Cr(s) | Cr3+(aq) || Sn2+(aq) | Sn(s) electrochemical cell if the concentration of Cr3+(aq) is 0.50 M and the concentration of Sn2+(aq) is 0.090 M. Report your answer to 3 significant figures.
Calculate the cell potential at 25°C for the Cr(s)|Cr3+(aq)||Sn²*(aq)|Sn(s) electrochemical cell if the concentration of Cr3+(aq) is o.50 M and the concentration of Sn²+(aq) is o.090 M. Report your answer to 3 significant figures. E cell V
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)
Calculate the potential for each cell as written at 25 °C. Indicate whether the metal electrode in the half-reaction opposite the standard hydrogen electrode, S.H.E., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely. S.H.E. || Zn²+ (aq, 0.0110 M)| Zn(s) Ecell = Pt(s) | V3+ (aq, 0.450 M), V²+ (aq, 0.00420 M) || S.H.E. Ecell = EZn²+ Zn Incorrect = -0.762 V V V E√3+√√²+ = -0.255 V

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For the reaction 2Co3+(aq)+2Cl(aq)->2Co2+(aq)+C12(g). Eocell=0.46 V what is the cell potential at 25 °C if the concentrations are [Co3+]=0.168mol L-1, [Co2+]=0.574mol L-1, and [CI-]-2.30\times 10-2mol L-1 and the pressure of Cl2 is PC12=9.70bar?