A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate the...
A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate the Gibbs free energy change at 25 °C when 2.61 g of iron is deposited. Assume the concentrations in the cell remain at the standard state values of 1 M through the entire deposition process.
Calculate the maximum amount of work done by the cell on its
surroundings.
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A Cr(s)|Cr3 (aq)||Fe3 (aq)|Fe(s) galvanic cell has a standard
cell potential of 0.700 V. Calculate the...
Half-reaction Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e - Fe(s) Fe3+ (aq) - Fe2+ (5)...
Half-reaction Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e - Fe(s) Fe3+ (aq) - Fe2+ (5) Sn+ (aq) + 2e - Sn2(aq) E (V) -0.74 -0.440 +0.771 +0.154 1. Calculate the standard cell potential for the voltaic cell based on the reaction below, given the table above: 35nt(s) + 2Cr (s) - 2 C (s) + 3 Sn () ANSWER: 2. Calculate the standard cell potential for the voltaic cell based on the reaction below, Riven the table above 3Feb...
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at...
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at 25 ∘C , given that [Fe3+]=0.00150 M and [Au3+]=0.795 M . Refer to the table of standard reduction potentials. E= V
A standard galvanic cell is constructed with Fe3+ | Fe2+and Cr3+ | Cr half cell compartments...
A standard galvanic cell is constructed with Fe3+ | Fe2+and Cr3+ | Cr half cell compartments connected by a salt bridge. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) Cr3+ is reduced at the cathode. As the cell runs, anions will migrate from the Cr3+|Cr compartment to the Fe3+|Fe2+compartment. Fe3+ is reduced at the cathode. The anode compartment is the Cr3+|Cr compartment. In the external circuit, electrons flow...
A CrCrN Ni galvanic cell is constructed in which the standard cell voltage is 0.490 V. Calculate ...
A CrCrN Ni galvanic cell is constructed in which the standard cell voltage is 0.490 V. Calculate the free energy change at 25°C when 0.907 g of Ni plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? Maximum work Submit Answer 3 question attempts remaining
A CrCrN Ni galvanic cell is constructed in...
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr(s) -0.74 Fe2+ (aq) + 2e- Fe (5) -0.440 Fe3+ (aq) + e - Fe2+ (s...
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr(s) -0.74 Fe2+ (aq) + 2e- Fe (5) -0.440 Fe3+ (aq) + e - Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. 35n4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq) A) +1.94 B) +0.89 C) +2.53 D) -0.59 E) -1.02
help with this one Construct a galvanic cell using the following half-reactions: Cr3+ (aq) + 3e - Cr(s) º = -0.56 V...
help with this one
Construct a galvanic cell using the following half-reactions: Cr3+ (aq) + 3e - Cr(s) º = -0.56 V 2 Hg2+(aq) + 2e - H922+(aq) = 0.92 V 2 Ho2+ The initial concentrations are: [Cr3+] =0.31 M [Hg2+] =2.57 M [Hg22+] =0.49 M (1) What is the potential of this non-standard cell at 298 K? Give your answer to 3 sig. figs. E(V) = Submit Answer Tries 0/2 (ii) How will each of the following changes to...
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq...
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) +...
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) + 2e- Fe () -0.440 Fe3+ (aq) + e- → Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. Cr (s) + 3Fe3+ (aq) + 3Fe2+ (aq) + Cr3+ (aq) A) -1.45 B) +2.99 C) +1.51 D) +3.05 E) +1.57
The standard half-cell potentials for three reactions are given below: Fe²+(aq) + 2e = Fe(s) Fe3+(aq)...
The standard half-cell potentials for three reactions are given below: Fe²+(aq) + 2e = Fe(s) Fe3+(aq) + 3e = Fe(s) Br2(aq) + 2e = 2Br (aq) E° = -0.44V E° = -0.04V E° = 1.09V Q 1(a) Determine what pair of half-cell reactions yields the most spontaneous redox process. Q 1(b) Calculate AGº for this process and comment on whether iron is plated during this process. Q 1(c) Draw a labelled energy level diagram showing the reactants, products and AGO....
Consider a galvanic cell that uses the half reactions: Fe3+(aq) + 3e → Fe(s) Ered=-0.04V Co2+...
Consider a galvanic cell that uses the half reactions: Fe3+(aq) + 3e → Fe(s) Ered=-0.04V Co2+ (aq) + 2e → Co(s) Ered - -0.28 V • 1) Calculate AGº for this reaction in kJ/mol. • 2) Calculate the equilibrium constant, K, for this reaction at 298 K • 3) What is the cell potential at 25°C when [Fe3+] - 1.09 M and [Co2+] = 0.057 M?
Half-reaction Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e - Fe(s) Fe3+ (aq) - Fe2+ (5) Sn+ (aq) + 2e - Sn2(aq) E (V) -0.74 -0.440 +0.771 +0.154 1. Calculate the standard cell potential for the voltaic cell based on the reaction below, given the table above: 35nt(s) + 2Cr (s) - 2 C (s) + 3 Sn () ANSWER: 2. Calculate the standard cell potential for the voltaic cell based on the reaction below, Riven the table above 3Feb...
A CrCrN Ni galvanic cell is constructed in which the standard cell voltage is 0.490 V. Calculate the free energy change at 25°C when 0.907 g of Ni plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? Maximum work Submit Answer 3 question attempts remaining
A CrCrN Ni galvanic cell is constructed in...
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr(s) -0.74 Fe2+ (aq) + 2e- Fe (5) -0.440 Fe3+ (aq) + e - Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. 35n4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq) A) +1.94 B) +0.89 C) +2.53 D) -0.59 E) -1.02
help with this one
Construct a galvanic cell using the following half-reactions: Cr3+ (aq) + 3e - Cr(s) º = -0.56 V 2 Hg2+(aq) + 2e - H922+(aq) = 0.92 V 2 Ho2+ The initial concentrations are: [Cr3+] =0.31 M [Hg2+] =2.57 M [Hg22+] =0.49 M (1) What is the potential of this non-standard cell at 298 K? Give your answer to 3 sig. figs. E(V) = Submit Answer Tries 0/2 (ii) How will each of the following changes to...
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) + 2e- Fe () -0.440 Fe3+ (aq) + e- → Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. Cr (s) + 3Fe3+ (aq) + 3Fe2+ (aq) + Cr3+ (aq) A) -1.45 B) +2.99 C) +1.51 D) +3.05 E) +1.57
The standard half-cell potentials for three reactions are given below: Fe²+(aq) + 2e = Fe(s) Fe3+(aq) + 3e = Fe(s) Br2(aq) + 2e = 2Br (aq) E° = -0.44V E° = -0.04V E° = 1.09V Q 1(a) Determine what pair of half-cell reactions yields the most spontaneous redox process. Q 1(b) Calculate AGº for this process and comment on whether iron is plated during this process. Q 1(c) Draw a labelled energy level diagram showing the reactants, products and AGO....
Consider a galvanic cell that uses the half reactions: Fe3+(aq) + 3e → Fe(s) Ered=-0.04V Co2+ (aq) + 2e → Co(s) Ered - -0.28 V • 1) Calculate AGº for this reaction in kJ/mol. • 2) Calculate the equilibrium constant, K, for this reaction at 298 K • 3) What is the cell potential at 25°C when [Fe3+] - 1.09 M and [Co2+] = 0.057 M?
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