Homework Answers
concentration cell contain both ions same with difference concentrations
Ecell = 0.05916 / n * log (higher / lower )
= 0.05916 / 2 * log (3.2 / 1.19 x 10^-2 )
= 0.07187 V
answer : 0.0719 V
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Two identical electrodes (A2+-A electrodes), where the half-reaction is A2+(aq) + 2e →A(s) E°= -0.852 V...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br2()+2e- 2Br (aq) HNO2(aqpH...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br2()+2e- 2Br (aq) HNO2(aqpH (aq)+ e-→ NO(g)+ H2O(I) standard reduction potential Ered1.065 v Erd- +1.00 V Answer the following questions about this cell Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
Refer to the following standard reduction half-cell potentials at 25∘C : VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V ...
Refer to the following standard reduction half-cell potentials at 25∘C : VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V Part A Part complete An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.017M)+2H+(aq,1.3M)+e−→→Ni2+(aq,2.5M)+2e−VO2+(aq,2.5M)+H2O(l) Calculate the cell potential under these nonstandard concentrations.
A voltaic cell is constructed with two Magnesium (Mg) electrodes. The two cell compartments have [Mg"]...
A voltaic cell is constructed with two Magnesium (Mg) electrodes. The two cell compartments have [Mg"] = 0.24 M and [Mgº'] = 0.53 M each respectively. The standard reduction potential for Mg (aq) + 2e → Mg (s) is -2.37 V. Predict whether the voltaic cell would proceed spontaneously.
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on...
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction: AgCI(s) teAg(s) + CI (aq) The two cell compartments have [CI] = 0.0 150 mol L-i and [Cl]-2.55 mol Li, respectively. 1. Which electrode is the cathode of the cell? 2. What is the standard EMF of the cell? 3. What is the cell EMF for the concentrations given? 4. For each electrode, predict if [CI] will increase, decrease, or stay...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Fe+3(aq)...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Fe+3(aq) +e− → Fe+2(aq) =E0red+0.771V 2H2O(l) +2e− → H2(g) + 2OH−(aq) =E0red−0.83V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you...
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
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s)...
Consider the 2 half-reactions: Cu2+(aq) + 2e- --> Cu(s) Eo= 0.34V Ag+(aq) + e- --> Ag(s) Eo= 0.8V If you increase the concentration of Cu2+(aq), which of the following would be true about the cell potential E? It would remain constant It would increase It would decrease This cannot be determined
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)...
Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e−...
Please show all steps taken (prefer typed solution)
Half-Reaction
E
°
(V)
Ag+ (aq) + e− → Ag (s)
0.7996
Al3+ (aq) + 3e− → Al (s)
−1.676
Au+ (aq) + e− → Au (s)
1.692
Au3+ (aq) + 3e− → Au (s)
1.498
Ba2+ (aq) + 2e− → Ba (s)
−2.912
Br2 (l) + 2e− → 2Br− (aq)
1.066
Ca2+ (aq) + 2e− → Ca (s)
−2.868
Cl2 (g) + 2e− → 2Cl− (aq)
1.35827
Co2+ (aq) + 2e−...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br2()+2e- 2Br (aq) HNO2(aqpH (aq)+ e-→ NO(g)+ H2O(I) standard reduction potential Ered1.065 v Erd- +1.00 V Answer the following questions about this cell Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do...
4. Zn2+(aq) + 2e Zn(s) E = -0.762 V Ag+ (aq) + e # Ag(s) E = 0.799 V Determine the voltage of the galvanic cell generated from these two half reactions, and calculate E of the cell when Zn2+ (aq) = 0.0100 M and Ag+ (aq) = 0.900 M at 25°C. Report the value of E
A voltaic cell is constructed with two Magnesium (Mg) electrodes. The two cell compartments have [Mg"] = 0.24 M and [Mgº'] = 0.53 M each respectively. The standard reduction potential for Mg (aq) + 2e → Mg (s) is -2.37 V. Predict whether the voltaic cell would proceed spontaneously.
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction: AgCI(s) teAg(s) + CI (aq) The two cell compartments have [CI] = 0.0 150 mol L-i and [Cl]-2.55 mol Li, respectively. 1. Which electrode is the cathode of the cell? 2. What is the standard EMF of the cell? 3. What is the cell EMF for the concentrations given? 4. For each electrode, predict if [CI] will increase, decrease, or stay...
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
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)...
Please show all steps taken (prefer typed solution)
Half-Reaction
E
°
(V)
Ag+ (aq) + e− → Ag (s)
0.7996
Al3+ (aq) + 3e− → Al (s)
−1.676
Au+ (aq) + e− → Au (s)
1.692
Au3+ (aq) + 3e− → Au (s)
1.498
Ba2+ (aq) + 2e− → Ba (s)
−2.912
Br2 (l) + 2e− → 2Br− (aq)
1.066
Ca2+ (aq) + 2e− → Ca (s)
−2.868
Cl2 (g) + 2e− → 2Cl− (aq)
1.35827
Co2+ (aq) + 2e−...
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