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Given that E degree = 0.52 V for the reduction Cu^2+ (aq) + e^- rightarrow Cu(s),...
Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate...
Given that E o = 0.52 V for the reduction Cu+(aq) + e− → Cu(s), calculate E o , ΔG o , and K for the following reaction at 25°C: 2Cu+(aq) ⇌ Cu2+(aq) + Cu(s) E o = V ΔG o = kJ K = × 10 Enter your answer in scientific notation.
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
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)...
If the value of E_cell^0 is 2.10 V for the reaction F_2 (g) + 2Fe^2+ (aq)...
If the value of E_cell^0 is 2.10 V for the reaction F_2 (g) + 2Fe^2+ (aq) rightarrow 2Fe^3+ (aq) + 2F^- (aq), what is the value of E_cell^0 for F^+ (aq) + Fe^3+ (aq) rightarrow Fe^2+ (aq) + 1/2 F_2 (g)? a. -4.20 V b -1.05 V c. 2.10V d. 1.05 V e. -2.10 V Given. Al^3+ (aq) + 3e^- Al(s); E^0 = -1.66 V Cl_2 (g) + 2e 2Cl^- (aq); E^0 = 1.36 V What is Delta G degree...
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...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate Delta S degree_univ given Delta S degree_sys = 179.1 J/K and Delta H degree_sys = -221.1 kJ.
Rh3+(aq) + 3e - Rh(s) E° = 0.80 V Cu (aq) + Cu(s) Eº - 0.52...
Rh3+(aq) + 3e - Rh(s) E° = 0.80 V Cu (aq) + Cu(s) Eº - 0.52 V What is the voltage of this cell if the concentrations of Cu and Rh3+ are each 1 M?
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^+] =
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.
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ...
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H 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
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)...
If the value of E_cell^0 is 2.10 V for the reaction F_2 (g) + 2Fe^2+ (aq) rightarrow 2Fe^3+ (aq) + 2F^- (aq), what is the value of E_cell^0 for F^+ (aq) + Fe^3+ (aq) rightarrow Fe^2+ (aq) + 1/2 F_2 (g)? a. -4.20 V b -1.05 V c. 2.10V d. 1.05 V e. -2.10 V Given. Al^3+ (aq) + 3e^- Al(s); E^0 = -1.66 V Cl_2 (g) + 2e 2Cl^- (aq); E^0 = 1.36 V What is Delta G degree...
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...
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate Delta S degree_univ given Delta S degree_sys = 179.1 J/K and Delta H degree_sys = -221.1 kJ.
Rh3+(aq) + 3e - Rh(s) E° = 0.80 V Cu (aq) + Cu(s) Eº - 0.52 V What is the voltage of this cell if the concentrations of Cu and Rh3+ are each 1 M?
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^+] =
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.
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...
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