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18 Nov 2019
Given the following spontaneous reaction occurring in an electrochemical cell under standard condition (25 degree C 1 atm, 1 mol/L...) 3 Cl_2(g) + 2 Fe(s) rightarrow 6 Cl^ - (aq) + 2 Fe^3+(aq) Eq-1 Cl_2(g) + 2s^ - rightarrow 2 Cl^ -(aq) E degree = + 1.36 V Eq.2 Fe^3+(aq) + 3e^ - rightarrow Fe(s) E degree = -0.04 V Eq.3 Write the cell notation when the above reaction Eq-1 serves as a battery rxn. Is Eq-1 a spontaneous rxn? Is it a redox rxn? Which species ar oxidant and reductant respectively? Use the standard half-cell potentials listed above to calculate the standard cell potential. What is the standard free energy change (delta G degree) of the battery reaction? If the above battery reaction reaches its equilibrium (a dead battery) then what is its equilibrium constant K?
Given the following spontaneous reaction occurring in an electrochemical cell under standard condition (25 degree C 1 atm, 1 mol/L...) 3 Cl_2(g) + 2 Fe(s) rightarrow 6 Cl^ - (aq) + 2 Fe^3+(aq) Eq-1 Cl_2(g) + 2s^ - rightarrow 2 Cl^ -(aq) E degree = + 1.36 V Eq.2 Fe^3+(aq) + 3e^ - rightarrow Fe(s) E degree = -0.04 V Eq.3 Write the cell notation when the above reaction Eq-1 serves as a battery rxn. Is Eq-1 a spontaneous rxn? Is it a redox rxn? Which species ar oxidant and reductant respectively? Use the standard half-cell potentials listed above to calculate the standard cell potential. What is the standard free energy change (delta G degree) of the battery reaction? If the above battery reaction reaches its equilibrium (a dead battery) then what is its equilibrium constant K?
Collen VonLv2
2 Sep 2019