Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C....
Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C.
O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq)
Br2(l)+2I−(aq)→2Br−(aq)+I2(s)
Homework Answers
![oxidation: 2x[Cu(s)-2e--> cu2+Cat.) ] 2.cu (0.401-034) v - O.06) V no. of electron exchanged、 Potantiat of ceu al) ca/En. -10](http://img.homeworklib.com/questions/18ed4e20-d6a6-11ea-ba94-d5a00bfe199c.png?x-oss-process=image/resize,w_560)
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Use tabulated half-cell potentials to calculate ΔG∘rxn
for each of the following reactions at 25 ∘C....
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Par...
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Part A Pb2+ (aq) +Mg(e)-Pb(a) +Mg (aq) VAZD AGn Submit Request Answer Part B Br ()+2Cl (aq)-+2Br (aq) + Cl( Express your answer using two significant figures AG Submit Request Answer Part C MnO2(a)+ 4H (aq) + Cu()Mn (ag) +2H,O( Express your answer using two significant figures
Calculate the equilibrium constant for each of the reactions at 25 ∘C. Standard Electrode Potentials at...
Calculate the equilibrium constant for each of the reactions at 25 ∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Pb2+(aq)+2e− →Pb(s) -0.13 Zn2+(aq)+2e− →Zn(s) -0.76 Br2(l)+2e− →2Br−(aq) 1.09 Cl2(g)+2e− →2Cl−(aq) 1.36 MnO2(s)+4H+(aq)+2e− →Mn2+(aq)+2H2O(l) 1.21 Pb2+(aq)+2e− →Pb(s) -0.13 Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) Express your answer using two significant figures.
Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. (F =...
Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. (F = 96,485 C/mol e) 2Li( s) + Cl 2 ( g) → 2 Cl - ( aq) + 2Li +( aq) Eº Li+(aq) + e- → Li(s) -3.04V Cl2 (g) + 2e- → 2 Cl- (aq) +1.36 V a. -425 kJ b. -849 kJ c. -8.49 x 10 5 kJ d. +324 kJ
Calculate the equilibrium constant for each of the reactions at 25∘C∘C. Standard Electrode Potentials at 25...
Calculate the equilibrium constant for each of the reactions at 25∘C∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction Cl2(g)+2e ---> 2CI- 1.36 I2(s)+2e --> 2I- 0.54 Part A Cl2(g)+2I−(aq)→2Cl−(aq)+I2(s) K= ?
se the tabulated half-cell potentials to calculate ??-for the following ,edo-m-mm in (7 points ) Tabulated...
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 tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reacti...
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I(aq) A.8.9 × 10-18 B.1.1 × 1017 C.1.7 × 1029 D.2.4 × 1058 E.3.5 × 10-59
Use the tabulated half-cell potentials below to calculate AG ( in Kilojoules for the following balanced...
Use the tabulated half-cell potentials below to calculate AG ( in Kilojoules for the following balanced redox reaction. F= 96,500 J/. mole e Pb2+(aq) + Cu(s) - Pb(s) + Cu2+(aq) Cu2+ (aq) + 2e -> Cu(s) E". Cu = -0.34 Volt Pb2+ (aq) + 2e-> Pb(s) E,Pb = -0.13 volt a. -41 kJ b. -81 kJ C. +46 kJ d. +91 kl e..91 kb 24 Calculate AS®rxn for the following reaction. The S' for each species is shown below the...
Use tabulated standard electrode potentials to calculate the standard cell potential for this reaction occurring in...
Use tabulated standard electrode potentials to calculate the standard cell potential for this reaction occurring in an electrochemical cell at 25 ∘C. Cr(s)+NO−3(aq)4H+(aq)→Cr3+(aq)+NO(g)+2H2O(l) Express your answer using two decimal places and include the appropriate units.
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced...
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s)+3 Mg2+(aq) A) 1.1 x 1072 B) 8.9 x 10-73 C) 1.1 x 10-72 D) 1.0 x 1024 E) 4.6 x 1031 2 Al3+(aq) +3 Mg(s)
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Part A Pb2+ (aq) +Mg(e)-Pb(a) +Mg (aq) VAZD AGn Submit Request Answer Part B Br ()+2Cl (aq)-+2Br (aq) + Cl( Express your answer using two significant figures AG Submit Request Answer Part C MnO2(a)+ 4H (aq) + Cu()Mn (ag) +2H,O( Express your answer using two significant figures
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 tabulated half-cell potentials below to calculate AG ( in Kilojoules for the following balanced redox reaction. F= 96,500 J/. mole e Pb2+(aq) + Cu(s) - Pb(s) + Cu2+(aq) Cu2+ (aq) + 2e -> Cu(s) E". Cu = -0.34 Volt Pb2+ (aq) + 2e-> Pb(s) E,Pb = -0.13 volt a. -41 kJ b. -81 kJ C. +46 kJ d. +91 kl e..91 kb 24 Calculate AS®rxn for the following reaction. The S' for each species is shown below the...
25) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s)+3 Mg2+(aq) A) 1.1 x 1072 B) 8.9 x 10-73 C) 1.1 x 10-72 D) 1.0 x 1024 E) 4.6 x 1031 2 Al3+(aq) +3 Mg(s)
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