1st Question:
The ΔG0 of a reaction is related to the cell potential(E0cell) as follows:
where n is the number of moles of electrons transferred in the cell reaction.
The E0cell of a reaction is given by:
where E0anode and E0cathode represents the standard reduction potentials of anode and cathode respectively.
Cathode is the half cell in which reduction happens. Here Pb2+ is getting reduced to Pb. Therefore Pb is the cathode. Therefore we have:
E0cathode = -0.13 V
Anode is the half cell in which oxidation happens. Here Cu is getting oxidized to Cu2+. Therefore Cu is the anode. Therefore we have:
E0anode = -0.34 V
Therefore we have:
Therefore we have:
E0cell = 0.21 V
n = 2 mole e (since 2 electrons are involved in the reaction)
F = 96500 J/V. mole e
Therefore ΔG0 of the reaction is:
Therefore the correct answer is the first option, that is:
a. -41 kJ
2nd Question:
The ΔS0rxn of a reaction is given by:
The ΔS0 of C2H3 is 24 J/mol.K
The ΔS0 of C4H2 is 18 J/mol.K
The ΔS0 of H2 is 3.0 J/mol.K
Therefore ΔS0rxn of the reaction is:
Therefore the correct answer is the first option, that is:
a. +24 J/K
Use the tabulated half-cell potentials below to calculate AG ( in Kilojoules for the following balanced...
30) Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) Pb2+(aq) + 2e → Pb(s) Cu2+ (aq) +2e → Cu(s) E° = -0.13 V E = 0.34 V C) 7.9 x 1015 A) 7.9 x 10-8 D) 1.3 x 10-16 B) 8.9 x 107 E) 1.1 x 10-8
ing Time: 2 hours, 12 min stion Completion Status: VULTIVITY Calculate ASºrxn for the following reaction. The sº for each species is shown below the action C4H2(g) + 2 H2(g) - 2C2H319) Given S°(J/mol K) 18 3.0 24 S°(J/mol K): C4H2= 18 : H2= 3.0: C2H3 = 24 O a. +24 J/K b. - 24J/K OC. 27 JK d.-27 J/K O e.-3.0 JK QUESTION 31 ams of aluminum( A.W = 27 g/mol) can be plated onto anche de
Calculate AS rxn for the following reaction. The S for each species is shown below the reaction. C4H2(g)+ 2 H2lg)2C2H3(g) Given: S°J/mol 'K) 18 3.0 24 surmorK) : C4H2" 18 ;·H2-3.0 ; C2H3-24 O a. +24 JK O b. 24 J/K ??. 27 JK d.-27 J/K Oe-3.0 J/K
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (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) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Using the standard reduction potentials given below, choose the reaction than can only be achieved through electrolysis. Cu2+(aq) + 2e → Cu(s) E° = 0.34 V Pb2+(aq) + 2e + Pb(s) E° = -0.13 V Fe2+(aq) + 2e Fe(s) E° = -0.44 V Zn2+(aq) + 2e + Zn(s) E° = -0.77 V Zn2+(aq) + Pb(s) → Zn(s) + Pb2+(aq) o Fe2+(aq) + Zn(s) → Fe(s) + Zn2+(aq) Pb2+(aq) + Fe(s) → Pb(s) + Fe2+(aq) Cu2+(aq) + Fe(s) → Cu(s) +...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
se the tabulated half-cell potentials to calculate ??-for the following ,edo-m-mm in (7 points ) Tabulated half-cell potentials (Reduction) Zar" (aq) + 2 e-? Zn(s) E.--0763 V Cl:(g) +2e2 CT(a)+1.358 F-96,485 C/mol. electron, 13-1 C.V and 1kJ -1000 C). (7 points) 4) Calculate K for the oxidation of copper by H' (at 25 Cu(s) + 2 r(aq) ? Cu2+(aq) + H2(g) Tabulated half-cell potentials (Reduction) Cu2 (aq) + 2 e-Al(s) E-0.34 v 2H+(aq) + 2 e--+ H2 (g) E#20.00 V...
Use the standard half-cell potentials listed below to calculate the standard free energy(K]for the following reaction occurring in an electrochemical cell at 25°C. Pb 2+ (aq) +2e--- Pb(s) E* - -0.13 Volt A13+ (aq) + 3 e-Al(s) E* =-1.66 volt a. 1.53 b. - 886 c-434 d. - 443 e. -1036 What is the standard free energy Gº) in Kilojoules for the reaction below at 298 Kelvin: Farady's constant = 96,485 joules/V. mole e Zn2+ (aq) + 2e ......> Zn(s)...