6. Calculate the equilibrium constant (K) for the following redox reaction at 25 ?C. Ecell =...
6. Calculate the equilibrium constant (K) for the following
redox reaction at 25 ?C. Ecell = -0.71 V
2 Al(s) + 3 Mg2+(aq) --> 2 Al3+(aq) + 3 Mg(s
Homework Answers
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6. Calculate the equilibrium constant (K) for the following
redox reaction at 25 ?C. Ecell =...
Use the provided reduction potentials to calculate the equilibrium constant (K) for the following balanced redox...
Use the provided reduction potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 °C: 2Al(s) + 3Mg2+(aq) → 2Al3+(aq) + 3Mg(s) E°(Al3+/Al) = -1.66 V and E°(Mg2+/Mg) = -2.37 V 1.0 × 1024 9.7 × 10-73 1.1 × 1072 4.6 × 1031 8.9 × 10-70
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced...
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s)+3 Mg2+(aq) A) 1.1 x 1072 B) 8.9 x 10-73 C) 1.1 x 10-72 D) 1.0 x 1024 E) 4.6 x 1031 2 Al3+(aq) +3 Mg(s)
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25...
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25 °C, E° Cd(s) + Cu 2+ (aq) → Cd 2+ (aq) + Cu(s)
6) Calculate the equilibrium constant K at 25°C for the following reaction for tant K at...
6) Calculate the equilibrium constant K at 25°C for the following reaction for tant K at 25°C for the following reaction for the standard cell potential (7 points) (nFEⓇ - RT In K, F=96485 C/mol.R=8.31 J/molk) Pb2+ (aq) + Fe(s) 5 Pb(8) + Fe²(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) | Fe*(aq) (1.1 M) || Cu?" (aq) (0.50 M) Cu() Ecell - Eºcell = 0.0592/n logQ
For the following redox reaction at 25 ºC, Eº cell = 2.24 V. Calculate the equilibrium...
For the following redox reaction at 25 ºC, Eº cell = 2.24 V. Calculate the equilibrium constant, K. Mg(s) + Pb 2+ (aq) → Mg 2+ (aq) + Pb(s)
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is...
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related...
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 where n 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. 0.34 Sn4t (aq)4eSn(s) 0.15...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n 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 Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reacti...
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo
1A) the equilibrium constant of reaction Sr(s)+Mg24(ac)---><--- Sr24(ac)+Mg(s) is 2.69X1012 at 25º C calculate the Eº...
1A) the equilibrium constant of reaction
Sr(s)+Mg24(ac)---><---
Sr24(ac)+Mg(s)
is 2.69X1012 at 25º C calculate the Eº of the cell
formed by the half cells Sr / Sr2 + and Mg / Mg2
+
R= 8.314 J/k -mol
F= 96500 J/V- mol
1B)
Calculate the standard emf of a cell using the Ag / Ag1 + and Al
/ Al3 + half-cell reactions.
answers
A)0.86 V
B)2.46 V
C)-1.86 V
D)-0.86 V
E cell AGⓇ =-nFEcell Ecell = F Ink AG°...
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s)+3 Mg2+(aq) A) 1.1 x 1072 B) 8.9 x 10-73 C) 1.1 x 10-72 D) 1.0 x 1024 E) 4.6 x 1031 2 Al3+(aq) +3 Mg(s)
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25 °C, E° Cd(s) + Cu 2+ (aq) → Cd 2+ (aq) + Cu(s)
6) Calculate the equilibrium constant K at 25°C for the following reaction for tant K at 25°C for the following reaction for the standard cell potential (7 points) (nFEⓇ - RT In K, F=96485 C/mol.R=8.31 J/molk) Pb2+ (aq) + Fe(s) 5 Pb(8) + Fe²(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) | Fe*(aq) (1.1 M) || Cu?" (aq) (0.50 M) Cu() Ecell - Eºcell = 0.0592/n logQ
Cell Potential and Equilibrium Standard reduction potentials The equilibrium constant, K, for a redox reaction is related to the standard cell potential, Ecel, by the equation Reduction half-reaction (V) Ag+ (aq) + e-→Ag(s) Cu2+ (aq) + 2e-→Cu(s) 0.34 Sn (a) 4e-Sn(s 0.15 2H' (aq) + 2e-→H2 (g) Ni2+ (aq) + 2e-→Ni(s)-0.26 Fe2+ (aq) + 2e-→Fe(s)-0.45 Zn2+ (aq) + 2e-→Zn(s)-0.76 Al3+ (aq) +3e-→Al(s) -1.66 Mg2+ (aq) + 2e-→Mg(s) -2.37 0.80 n FEcell where n is the number of moles of electrons...
Review I Constants I Periodic Table The equilibrium constant, K, for a redox reaction is related to the standard potential, E°, by the equation Standard reduction potentials nFE RT In K E° (V) Reduction half-reaction Agt(aq)eAg(s) Cu2+(aq)2eCu(s) 0.80 where n 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. 0.34 Sn4t (aq)4eSn(s) 0.15...
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n 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 Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo
1A) the equilibrium constant of reaction
Sr(s)+Mg24(ac)---><---
Sr24(ac)+Mg(s)
is 2.69X1012 at 25º C calculate the Eº of the cell
formed by the half cells Sr / Sr2 + and Mg / Mg2
+
R= 8.314 J/k -mol
F= 96500 J/V- mol
1B)
Calculate the standard emf of a cell using the Ag / Ag1 + and Al
/ Al3 + half-cell reactions.
answers
A)0.86 V
B)2.46 V
C)-1.86 V
D)-0.86 V
E cell AGⓇ =-nFEcell Ecell = F Ink AG°...
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