Calculate the Standard Cell Potential for a Pb acid battery and for a H2 fuel cell.
Calculate the Standard Cell Potential for a Pb acid battery and for a H2 fuel cell.
The standard half-cell reactions of lead acid battery is: 2) Half-cell reduction reaction form: red 1.69 +4Ht +so +2ePbSO4,()+2H2O) РЬОог.0) Red (aq) -Ox. PbSO4.()+2e Pb)+SO -0.36 4.(aq) Pb()+PbO2.(s)+2H2SO4.(ag) Tot. 2PBSO4.()+ 2H20() 2.05 a) Determine the full cell reaction of lead acid batter and the total cell potential when discharging the battery. I b) The half-cell potentials are given according to a reference potential. Describe this reference potential. What is the point of a reference potential?
The standard cell potential for the fuel cell 2 H2(g) + O2(g) ⇔ 2 H2O(l) is = +1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy change of the cell reaction.
The standard half-cell reactions of lead acid battery is: 2) ЕФN Half-cell reduction reaction form: red PbOo2.(s) 4H+ + so2 4, (aq) PbSO4,()+2H20 Red 2e 1.69 Рo) + So?- 4.(aq) -Ox -0.36 Pbs04.(s)2e Pb()PbO2,(s)+ 2H2SO4,(ag) 2P6SO4.(6) +2H20D 2.05 Tot. a) Determine the full cell reaction of lead acid batter and the total cell potential when discharging the battery b) The half-cell potentials are given according to a reference potential. Describe this reference potential. What is the point of a reference...
The standard cell potential for the fuel cell 2 H2(g) + O2(g) → 2 H2O(l) is E° = +1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy change of the cell reaction. Use Table 7.1. to determine v (E-E) A. Sº = vF 7. 0 -160 J mol-1 K-1 0-320 J mol-1 k-1 O-107 J mol-1 K-1 0 -80 J mol-1 k-1
In the following cell, A is a standard Pb2+|Pb electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.13 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Pb2+/Pb couples are 0.00 and -0.13 V, respectively. voltmeter saltbridge 1+ Pl(s) LPH2 (g) O Pb2+(aq) + H2(g) --> Pb(s) + 2H+(aq) O Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g)
Calculate the cell potential of a cell composed of a cathode consisting of a Pb wire immersed in a 1.14 M Pb2+ solution and an anode consisting of a Pb wire immersed in a 2.10×10-5 M Pb2+ solution. Assume the temperature of the solutions is 298 K. Cell potential: V
In a hydrogen fuel cell, oxygen and hydrogen are combincd to produce water and a small potential differ- ence. The steps of the chemical reaction are: at-electrode: at + electrode: H2 + 20H-→ 2H2O + 2e-; O2 + H2O + 2e-→ 2OH-, Use the table of chemical values to calculate a) the work that can be produced from this fuel cell, b) the 'waste' heat produced during standard operation, c) the voltage of the cell, and d) the minimum voltage...
In the following cell, A is a standard Pb2+|Pb
electrode connected to a standard hydrogen electrode. If the
voltmeter reading is –0.13 V, match each electrode with its correct
name.
Given: Standard reduction potential of the
H+/H2 and Pb2+/Pb couples are 0.00
and –0.13 V, respectively.
Question 2 options:
12
Pb2+|Pb electrode
12
standard hydrogen electrode
1.
anode
2.
cathode
Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential below, Cut2 (aq) + 2 e. ----> Cu (s) ° = 0.337 volts Pb+2 (aq) + 2 e--...-> Pb(s) ° = -0.126 volts 0.211 V 0.463 V -0.463 V -0.211 V In Part III, to light up a white LED bulb will require forward voltage (VF) at 20 mA. • 5 1.2. 2.0 Calculate the cell potential difference, Eºcell ( cell = Eºcathode -...
Use the Nernst euation and the cell potential for the Pb-PbI2 cell and the known [Pb2+] to calculate the [Pb2+] in equilibrium with PbI2. The measured avgerage cell potential of Pb-PbI2 is 0.084 V the known [Pb2+] is 0.050 M Eo of Pb2+ (aq) + 2 e- --------> Pb(s) is -0.13 V 0.050 M KI Mixed 9 mL of 0.050 M KI with 3 mL of 0.050 M Pb(NO3)2 .