Zn(s) ------------> Zn^2+(aq) + 2e^- E0 = 0.76v
Cl2(g) + 2e^- -------> 2Cl^-(aq) E0 = 1.362v
---------------------------------------------------------------------------
Zn(s) + Cl2(g) -------> Zn^2+(aq) + 2Cl^- (aq) E0 = 2.122v
n = 2
[Zn^2+] = 0.01M
PCl2 = 4atm
[Cl^-] = 1M
E = E0 -0.0592/n logQ
= 2.122-0.0592/2 log[Cl^-]^2[Zn^2+]/PCl2
= 2.122-0.0296log(1)^2*0.01/4
= 2.122-0.0296log0.0025
= 2.122-0.0296*-2.6020
= 2.2v >>>>answer
Use the Nernst equation to calculate the corresponding voltage if the Cl (9) were at 4.0...
Constants Periodic Table РапA The Nernst equation is the one of the most important equations in electrochemistry. At standard temperature, 25 °C or 298 K, the equation has the form E=E° – (0.0591 ) logQ For the reaction 2CO3+ (aq) + 2Cl(aq) +2Co2+ (aq) + C1, (g). E=0.71 V what is the cell potential at 25°C if the concentrations are Co3] =0.728 M, Co2+] = 0.143 M, and [Cl] =0.116 M and the pressure of Cl2 is Pci, = 5.60...
+ The Nernst Equation 4 of 5 A Review Constants Periodic Ta The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is Part A EN E 2.303 RT 10g10 Q For the reaction where E is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred,...
Use the table of Standdard Reduction Potentials and the Nernst
Equation to calculate the concentration of Cu2+ present in the
Cu/Cu2+ half-cell after the addition NH3 (aq) while it was coupled
with
a) Zn/Zn2+
b) Ag/Ag+
Table 2 has your measured voltages for these cells. SHOW YOUR
SETUP OF THE NERST EQUATION WITH ALL VARIABLES FILLED IN. SHOW THE
CALCULATED [Cu2+] CONCENTRATION.
Table 2:
METAL
Mg
Ag
Ni
Zn
Pb
Cu
1.230 V
0.642 V
0.030 V
0.648 V
0.256...
The Nernst equation is the one of the most important equations in electrochemistry. At standard temperature, 25 ∘C or 298 K, the equation has the form E=E∘−(0.0591n)logQ where E∘ is the standard reduction potential for the reaction in volts and Q is the reaction quotient. The reaction quotient has the usual form Q=[products]x[reactants]y A table of standard reduction potentials gives the voltage at standard conditions, 1.00 Mfor all solutions and 1.00 atm for all gases. The Nernst equation allows for...
Part A
Please show all of the steps.
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard- state conditions, the equation is E = E – 2.303 RT logo ne where is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q...
this is the complete question (no more info)
Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e --> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e --> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e --> Ni(s); E° =...
Constants Periodic Table The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard- state conditions, the equation is Part A E= E° – 2.303 RT 1000 RT log10 Q nF where E is the potential in volts, Eº is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q...
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is Part A E E- 2.303 RT logO For the reaction nF 2C03 (aq)2Ci (aq)+2C02+ (aq) Cl2 (g). E = 0.483 V where E is the potential in volts, E° is the standard potential in volts, R is the gas constant, T what is the cell potential at 25 °C if the concentrations are Co3+ M, and the...
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