Homework Answers
(6)
Here Al is getting oxidized and Cu is getting reduced.
E0cell = Eoxid + Ered = 1.662 + 0.337 = 1.999 V
(b)
False.
Because E0cell > 0 which means cell reaction is spontanoeus.
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Determine the standard cell potential (in volts) at 25 degree C for the following reaction. You...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
Given the measured cell potential, E_cell, is -0.3657 V at 25 degree C in the following...
Given the measured cell potential, E_cell, is -0.3657 V at 25 degree C in the following cell, calculate the H^+ concentration Pt (s)|H_2(g, 0.801 atm)|H^+ (aq, ? M)||Cd^2+ (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E degree, are as follows. 2H^+ (aq) + 2e^- rightarrow H_2 (g) E degree = 0.00 V Cd^2+ (aq) + 2e^- rightarrow Cd (s) E degree = -0.403 V [H^+] =
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) +...
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) + 2e —>H2 (1.68atm) The reduction potential for the following non-standard half cell at 298K is volts. Al3+ (4.93x10-*M)+ 3e —AI (S) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 6.44x10 atm, the F concentration is 1.41M, and the Ni2+ concentration is 1.28M? F2(g) + Ni(s)— 2F" (aq) +...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g),...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g), Delta G degree = -31.0 kJ consider the galvanic cell that uses the reaction 2 Ag^+ (aq) plus Cu(s) rightarrow Cu^2+ (aq) + 2Ag (s) clearly sketch the experimental set-up, write down the anode and cathode half- give the shorthand notation for the cell For the following cell, write a balanced equation for the cell reaction and calc Delta G degree C: Pt(s) |H_2(1.0...
Calculate the cell potential for the following reaction as written at 25.00 degree C. given that...
Calculate the cell potential for the following reaction as written at 25.00 degree C. given that [Cr^2+] = 0.893 M and [Ni^2+] = 0.0110 M. Standard reduction potentials can be found here. Cr(s)+Ni^2+(aq) Cr^2+(aq)+Ni(s)
Calculate the cell potential for the following reaction as written at 25.00 degree C, given that...
Calculate the cell potential for the following reaction as written at 25.00 degree C, given that [Zn^2+] = 0.875 M and [Fe^2+] = 0.0160 M. Standard reduction potentials can be found here. Zn(s) + Fe^2+(aq) reversible Zn^2+ (aq) + Fe(s) E = V
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+...
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+ (aq, 0.50 M)||I^- (aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e^- rightarrow Ag(s) + I^-(aq) E degree = -0.15 V Sn^4+ (aq) + 2 e^- rightarrow SN^2+ (aq) E degree= +0.15 V.
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an el...
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as...
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as written). Identify each oxidizing agent and reducing agent. Ni (s) + Zn2+(aq) ----> Ni2+(aq) + Zn (s) Ni (s) + Pb2+(aq) -------> Ni2+(aq) + Pb (s) Al (s) + 3 Ag+(aq) ---------> Al3+(aq) + Ag (s) Pb (s) + Mn2+(aq) ----------> Pb2+(aq) + Mn (s)
Given the following standard reduction potentials: H^+ (aq) + 2e^- rightarrow H_2(g) E degree = 0.00...
Given the following standard reduction potentials: H^+ (aq) + 2e^- rightarrow H_2(g) E degree = 0.00 V Fe^3+ (aq) + 2e^- rightarrow Fe(s) E degree = -0.43 V (a) What is the cell potential by combining the above two half-reactions to make a working voltaic cell (same as galvanic cell)? (b) Which species will be oxidized in anode? Write the half-reaction for the anode. (c) Write the overall reaction and balance the chemical equation for this working voltaic cell. (d)...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
Given the measured cell potential, E_cell, is -0.3657 V at 25 degree C in the following cell, calculate the H^+ concentration Pt (s)|H_2(g, 0.801 atm)|H^+ (aq, ? M)||Cd^2+ (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E degree, are as follows. 2H^+ (aq) + 2e^- rightarrow H_2 (g) E degree = 0.00 V Cd^2+ (aq) + 2e^- rightarrow Cd (s) E degree = -0.403 V [H^+] =
The reduction potential for the following non-standard half cell at 298K is volts. 24+ (1.83x10-3M) + 2e —>H2 (1.68atm) The reduction potential for the following non-standard half cell at 298K is volts. Al3+ (4.93x10-*M)+ 3e —AI (S) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 6.44x10 atm, the F concentration is 1.41M, and the Ni2+ concentration is 1.28M? F2(g) + Ni(s)— 2F" (aq) +...
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g), Delta G degree = -31.0 kJ consider the galvanic cell that uses the reaction 2 Ag^+ (aq) plus Cu(s) rightarrow Cu^2+ (aq) + 2Ag (s) clearly sketch the experimental set-up, write down the anode and cathode half- give the shorthand notation for the cell For the following cell, write a balanced equation for the cell reaction and calc Delta G degree C: Pt(s) |H_2(1.0...
Calculate the cell potential for the following reaction as written at 25.00 degree C. given that [Cr^2+] = 0.893 M and [Ni^2+] = 0.0110 M. Standard reduction potentials can be found here. Cr(s)+Ni^2+(aq) Cr^2+(aq)+Ni(s)
Calculate the cell potential for the following reaction as written at 25.00 degree C, given that [Zn^2+] = 0.875 M and [Fe^2+] = 0.0160 M. Standard reduction potentials can be found here. Zn(s) + Fe^2+(aq) reversible Zn^2+ (aq) + Fe(s) E = V
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+ (aq, 0.50 M)||I^- (aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e^- rightarrow Ag(s) + I^-(aq) E degree = -0.15 V Sn^4+ (aq) + 2 e^- rightarrow SN^2+ (aq) E degree= +0.15 V.
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Given the following standard reduction potentials: H^+ (aq) + 2e^- rightarrow H_2(g) E degree = 0.00 V Fe^3+ (aq) + 2e^- rightarrow Fe(s) E degree = -0.43 V (a) What is the cell potential by combining the above two half-reactions to make a working voltaic cell (same as galvanic cell)? (b) Which species will be oxidized in anode? Write the half-reaction for the anode. (c) Write the overall reaction and balance the chemical equation for this working voltaic cell. (d)...
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