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Calculate the standard emf value for the following reaction if K = 4.58 x 1015 at...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) Pb2+(aq) + 2e → Pb(s) Cu2+ (aq) +2e → Cu(s) E° = -0.13 V E = 0.34 V C) 7.9 x 1015 A) 7.9 x 10-8 D) 1.3 x 10-16 B) 8.9 x 107 E) 1.1 x 10-8
1. What is the value (in V) of Eocell for the following reaction? Co2+ (aq) +...
1. What is the value (in V) of Eocell for the following reaction? Co2+ (aq) + Be (s) → Co (s) + Be2+ (aq) 2.What is Eocell (in V) for a redox reaction where one electron is transferred with an equilibrium constant (K) of 1.44 x 10-14? 3.Consider the following reaction: Cu2+ (aq) + Pb (s) → Cu (s) + Pb2+ (aq) What will be Ecell for this reaction (in V) when [Cu2+] = 0.500 M and [Pb2+] = 0.0350...
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
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions...
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction...
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction occurring in an electrochemical cell at 25°C. Pb 2+ (aq) +2e--- Pb(s) E* - -0.13 Volt A13+ (aq) + 3 e-Al(s) E* =-1.66 volt a. 1.53 b. - 886 c-434 d. - 443 e. -1036 What is the standard free energy Gº) in Kilojoules for the reaction below at 298 Kelvin: Farady's constant = 96,485 joules/V. mole e Zn2+ (aq) + 2e ......> Zn(s)...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) +...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0007 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 Li+(aq) + 1 Sn(s) --> 2 Li(s) + 1 Sn2+(aq) (b) 1 Zn2+(aq) + 1 Ca(s) --> 1 Zn(s) + 1 Ca2+(aq) (c) 1 Mg2+(aq)...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 H+(aq) + 2 Cu(s) --> 1 H2(g) + 2 Cu+(aq) E = V (b) 1 Ca2+(aq) + 2 K(s) --> 1 Ca(s) + 2 K+(aq) E...
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
Consider the following reaction at 298 K: 3Cu2+(aq) + 2Al(s) + 3Cu(s) + 2 A13+ (aq)...
Consider the following reaction at 298 K: 3Cu2+(aq) + 2Al(s) + 3Cu(s) + 2 A13+ (aq) and the standard reduction potential values: Cu2+(aq) + 2e + Cu(3) E° = +0.342 v Al3+ (aq) + 3e + Al(s) E° = -1.662 v No files uploaded (Submit 6.1 and 6.2 as a single file) Q6.1 8 Points Calculate the standard Gibbs energy of reaction (A,G), in kJ/mol. Q6.2 8 Points Calculate the emf (E) when [Cu2+] = 1.0 x 10-2 M and...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) Pb2+(aq) + 2e → Pb(s) Cu2+ (aq) +2e → Cu(s) E° = -0.13 V E = 0.34 V C) 7.9 x 1015 A) 7.9 x 10-8 D) 1.3 x 10-16 B) 8.9 x 107 E) 1.1 x 10-8
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
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction occurring in an electrochemical cell at 25°C. Pb 2+ (aq) +2e--- Pb(s) E* - -0.13 Volt A13+ (aq) + 3 e-Al(s) E* =-1.66 volt a. 1.53 b. - 886 c-434 d. - 443 e. -1036 What is the standard free energy Gº) in Kilojoules for the reaction below at 298 Kelvin: Farady's constant = 96,485 joules/V. mole e Zn2+ (aq) + 2e ......> Zn(s)...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
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
Consider the following reaction at 298 K: 3Cu2+(aq) + 2Al(s) + 3Cu(s) + 2 A13+ (aq) and the standard reduction potential values: Cu2+(aq) + 2e + Cu(3) E° = +0.342 v Al3+ (aq) + 3e + Al(s) E° = -1.662 v No files uploaded (Submit 6.1 and 6.2 as a single file) Q6.1 8 Points Calculate the standard Gibbs energy of reaction (A,G), in kJ/mol. Q6.2 8 Points Calculate the emf (E) when [Cu2+] = 1.0 x 10-2 M and...
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