Homework Answers
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are...
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are rechargeable. The relevant half-cell reactions for such batteries are given in this table. Half-Reaction, Cd(OH)2(s) + 2e- -> Cd(s) + 2 OH- (aq) E(volts) = -0.809 NiOOH(s)+ H2O(l) + e- -> Ni(OH)2(s)+OH-(aq) E(volts) = +0.490 A) Write a balanced equation for the process that produces electricity in a nicad battery and specify the half- reaction that occurs at the anode. B) Calculate the potential expected...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s)...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Help with Part C please? Not sure if I have the correct information to determine an answer
Help with Part C please? Not sure if I have the correct
information to determine an answer
Problems 1. Given the standard reduction potentials Cd(OH)2(s) +2e → Cd(s) + 2 OH-(aq) В"--0.76 V Ni0(OH)(s) + H20() + r-, Ni(OH)2(s) + OH-(aq) E。_ +0.49 V Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. a. b. Calculate the standard potential of this battery. A typical nicad battery has a potential of 1.30 V. Why is there a...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Ecd=-0.13...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Ecd=-0.13 V Cro2 (aq)+4 H2O(1)+3e" → Cr(OH)3(s)+50H (aq) Cu2+ (aq)+e → Cut(aq) = +0.153 V Answer the following questions about this cell. 0-0 Write a balanced equation for the half-reaction that happens at the cathode. DI X 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...
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s)...
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s) E = +0.80 V Sn2+ (aq) + 2 e Sn(s) E = -0.14 V Identify the anode and give the cell voltage under standard conditions: O A Sn: Eºcell = -0.66 V B. Sn; Eºcell = 0.66 V O C. Ag: Eºcell = 0.67 V D. Ag: Eºcell = 0.94 V E. Sn; Eºcell = 0.94 V
Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s) Q3\ For the previous cell,...
Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s) Q3\ For the previous cell, determine the concentration of the cobalt ion when a cell voltage of 1.76 V is obtained using a 0.761 M gold (III) nitrate solution. Q4\ Calculate the free energy for the nonstandard cell in the previous problem. Show all work. Be mindful of signs, sig figs, and units Q5\ Consider a galvanic cell consisting of the following two redox couples: Sn2+ (aq, 0.010 M)...
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e...
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e -0.26 V Ni (s) Cd (s) Reduction Ni (8) Ereduction Cd (8) Ereduction Ni2+ (aq) Cd2+ (aq) Oxidation Salt Bridge Look at the voltaic cell diagram above and finish the following sentences using options given on the table above: i) Ais ii) B is metal on the left metal on the right solution on the left iii) Cis iv) Dis solution on the right...
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using...
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using the following standard reduction potentials. Ag+(aq) + e- → Ag(s) E° = 0.80 V Ca2+(aq) + 2e + Ca(s) E° = -2.87 V 2.07 V -3.67 V 3.67 V -2.29 V -2.07 V
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai...
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai (aq)3eAl (s) Eo0.7996 V E0.342 V Eo-1.6632 V i. Which pair of half reactions would make the battery with the largest E cell? i. Identify the cathode and the anode for this battery, and calculate the value of E cell. i. Write the overall redox reaction that would take place in the battery above.
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
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Help with Part C please? Not sure if I have the correct
information to determine an answer
Problems 1. Given the standard reduction potentials Cd(OH)2(s) +2e → Cd(s) + 2 OH-(aq) В"--0.76 V Ni0(OH)(s) + H20() + r-, Ni(OH)2(s) + OH-(aq) E。_ +0.49 V Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. a. b. Calculate the standard potential of this battery. A typical nicad battery has a potential of 1.30 V. Why is there a...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Ecd=-0.13 V Cro2 (aq)+4 H2O(1)+3e" → Cr(OH)3(s)+50H (aq) Cu2+ (aq)+e → Cut(aq) = +0.153 V Answer the following questions about this cell. 0-0 Write a balanced equation for the half-reaction that happens at the cathode. DI X 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...
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s) E = +0.80 V Sn2+ (aq) + 2 e Sn(s) E = -0.14 V Identify the anode and give the cell voltage under standard conditions: O A Sn: Eºcell = -0.66 V B. Sn; Eºcell = 0.66 V O C. Ag: Eºcell = 0.67 V D. Ag: Eºcell = 0.94 V E. Sn; Eºcell = 0.94 V
Anode E A Cathode B 7 С D Ni2+ + 2e -0.40 V Cd2+ + 2e -0.26 V Ni (s) Cd (s) Reduction Ni (8) Ereduction Cd (8) Ereduction Ni2+ (aq) Cd2+ (aq) Oxidation Salt Bridge Look at the voltaic cell diagram above and finish the following sentences using options given on the table above: i) Ais ii) B is metal on the left metal on the right solution on the left iii) Cis iv) Dis solution on the right...
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using the following standard reduction potentials. Ag+(aq) + e- → Ag(s) E° = 0.80 V Ca2+(aq) + 2e + Ca(s) E° = -2.87 V 2.07 V -3.67 V 3.67 V -2.29 V -2.07 V
5. Consider the following set of half reactions Ag (aq)Ag (s) Cu2(a)2 e- Cu (s) Ai (aq)3eAl (s) Eo0.7996 V E0.342 V Eo-1.6632 V i. Which pair of half reactions would make the battery with the largest E cell? i. Identify the cathode and the anode for this battery, and calculate the value of E cell. i. Write the overall redox reaction that would take place in the battery above.
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
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