Homework Answers
18. Reverse the reaction and divide by 2,
Eocell = (-2.10V)/2 = -1.05V ,
so option b) is the answer
19. 2 Al+3 + 6e- -------> 2Al ;
Eo = 2*(-1.66) = -3.32V
6 Cl- ---------> 3Cl2 + 6e- ;
Eo = 3*(-1.36) = -4.08V
Add these 2 above equations to get the overall 9eqn
given in the question)
Eocell = Ecathode -
Eanode
ΔGo=-nFEocell , use these formulas
to get the answer
20) At room temperature,
Ecell = Eocell -
0.0592/n log [Ox]/[Red]
Ecell = 0.460 - 0.0592/2 log (0.017 /
0.18)
Ecell = 0.4903 V option d)
21) electrons deposited = it /F = (15*160*60 sec) / 96485 C/mol =
1.49245 mole of electrons
1.49245 * (1 mole of Cr / 3moles of elcrons) = 0.49748
mol of Cr
mass of Cr deposited = 0.49748 mol of Cr * 51.99
gm/mol = 25.86 gms = 25.89 gms approx
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If the value of E_cell^0 is 2.10 V for the reaction F_2 (g) + 2Fe^2+ (aq)...
Given that E degree = 0.52 V for the reduction Cu^2+ (aq) + e^- rightarrow Cu(s),...
Given that E degree = 0.52 V for the reduction Cu^2+ (aq) + e^- rightarrow Cu(s), calculate E degree delta G degree, and K for the following reaction at 25 degree C: 2 Cu^+ (aq) rightwardsharpoonoverleftwardsharpoon Cu^2+ (aq) + Cu(s) E degree = V delta G degree = kJ K = times 10 Enter your answer in scientific notation.
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^+] =
K_p for NH_3 at 25 degree C N_2 (g) + 3 H_2(g) irreversible 2 NH_3 (g),...
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1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq)...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq) + 2I-1(aq) E = ? a.-0.87 V b.-0.19 V c.0.19 V d.0.87 V 2) Calculate the equilibrium constant (Keq) for the following reaction at 25 °C? (Faraday's Constant = 96,500 J / V · mol) & (R = 8.314 J / mol · K) 2Fe+3(aq) + Sn+2(aq) → 2Fe+2(aq) + Sn+4(aq) K = ? a. 4.04 x 107 b. 3.44 x 1018 c. 4.48...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standar...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standard potential for the cell reaction for 2 Ag + H2 (g)-2 Ag+2H +0.80 V b. a. +0.40 V +0.12 V d. c. -0.12 v none of these e. 40. Given: Fe (s) + 2 Ag' (aq) Fe (ag)+ 2 Ag (s) with E ell -1.24 V What is the...
please help, thanks! 7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq)...
please help, thanks!
7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq) a. Cd Cd| Ni | Ni d. Ni Cd I N | Ca b. Cd CdNi | Ni e. Cd |Cd Ni Ni 8. Calculate AS for the dissociation of dinitrogen tetraoxi de at 25°C NOdg) 2NO:(g) AG, J/mol)AH, J/mol) Substance NO) NOdg) +33.2 +51.3 +97.9 +9.2 d. +0.076 kJ K a.-2.10 kJ/K e +2.10kJ/K b. -0.550 kJ/K c.-0.208 kJ/K 9. Use the standard...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b)...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b) precipitation reaction oxidation-reduction reaction d) acid-base neutralization reaction 9. c) single replacement What is the volume of 0.1220 M HNO, solution required to completely neutralize 17.50 ml of 0.1211M NAOH? Reaction is: HNO, (aq) + NaOH(aq) -NaNO, (aq) + H:0 (aq) a) 17.37 ml b) 16.31 ml. c) 15.39 ml. d) 17.84 mL 10. Which one of the following reactions is the reduction reaction?...
Please show your work Given the following standard reduction potentials, Ag^+(aq) + e^- rightarrow Ag(s) E^degree...
Please show your work
Given the following standard reduction potentials, Ag^+(aq) + e^- rightarrow Ag(s) E^degree = 0.80 V AgCN(s) + e^- rightarrow Ag(s) + CN^-(aq) E^degree = -0.01 V calculate the solubility product of AgCN at 25degree C. A) 4.3 time 10^-14 B) 2.3 times 10^13 C) 2.1 time 10^*-14 D) 5.1 times 10^13 E) None of these
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Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
What is the value of Δ G° (in kJ ) for the following balanced redox reaction at 25.0℃ ?
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Given that E degree = 0.52 V for the reduction Cu^2+ (aq) + e^- rightarrow Cu(s), calculate E degree delta G degree, and K for the following reaction at 25 degree C: 2 Cu^+ (aq) rightwardsharpoonoverleftwardsharpoon Cu^2+ (aq) + Cu(s) E degree = V delta G degree = kJ K = times 10 Enter your answer in scientific notation.
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^+] =
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...
39. Given: E +0.46 V Eo- +0.34 V Cu(s) + 2 Ag+ → 2 Ag (s) + Cu2. Cu2+ + H2 (g) → Cu (s) + 2 H' Find the standard potential for the cell reaction for 2 Ag + H2 (g)-2 Ag+2H +0.80 V b. a. +0.40 V +0.12 V d. c. -0.12 v none of these e. 40. Given: Fe (s) + 2 Ag' (aq) Fe (ag)+ 2 Ag (s) with E ell -1.24 V What is the...
please help, thanks!
7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq) a. Cd Cd| Ni | Ni d. Ni Cd I N | Ca b. Cd CdNi | Ni e. Cd |Cd Ni Ni 8. Calculate AS for the dissociation of dinitrogen tetraoxi de at 25°C NOdg) 2NO:(g) AG, J/mol)AH, J/mol) Substance NO) NOdg) +33.2 +51.3 +97.9 +9.2 d. +0.076 kJ K a.-2.10 kJ/K e +2.10kJ/K b. -0.550 kJ/K c.-0.208 kJ/K 9. Use the standard...
8 The Following reaction is classified as: 2HCl(aq) + Ba(OH)2(aq) → BaCl(aq) + 2 H20(0) b) precipitation reaction oxidation-reduction reaction d) acid-base neutralization reaction 9. c) single replacement What is the volume of 0.1220 M HNO, solution required to completely neutralize 17.50 ml of 0.1211M NAOH? Reaction is: HNO, (aq) + NaOH(aq) -NaNO, (aq) + H:0 (aq) a) 17.37 ml b) 16.31 ml. c) 15.39 ml. d) 17.84 mL 10. Which one of the following reactions is the reduction reaction?...
Please show your work
Given the following standard reduction potentials, Ag^+(aq) + e^- rightarrow Ag(s) E^degree = 0.80 V AgCN(s) + e^- rightarrow Ag(s) + CN^-(aq) E^degree = -0.01 V calculate the solubility product of AgCN at 25degree C. A) 4.3 time 10^-14 B) 2.3 times 10^13 C) 2.1 time 10^*-14 D) 5.1 times 10^13 E) None of these
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
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