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![- 0 =k = equilibrium constant. According to Nernst equation, E = CO - RI in [product] Creactant At equilibrium , [product] [](http://img.homeworklib.com/questions/8eacc370-dc38-11eb-b6e9-5df82963106a.png?x-oss-process=image/resize,w_560)
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Question 22 of 33 What is the equilibrium constant K at 25°C for an electrochemical cell...
What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0140...
What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0140 V and n = 2? (F = 96,500 J/(V•mol), R = 8.314 J/ (mol·K)) 0.3353 1 2 3 x 4 5 6 с 7 00 9 O +/- x 100 Complete and balance the following redox reaction in basic solution MnO4 (aq) + C2042-(aq) → MnO2 (s) + CO2(g) 3C22 Reset < > х 1 2 3 4 5 6 7 8 9 0...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq)...
1) Calculate the cell potential, E°cell, for the following electrochemical reaction. Cu(s) + I2(g) → Cu+2(aq) + 2I-1(aq) E = ? a.-0.87 V b.-0.19 V c.0.19 V d.0.87 V 2) Calculate the equilibrium constant (Keq) for the following reaction at 25 °C? (Faraday's Constant = 96,500 J / V · mol) & (R = 8.314 J / mol · K) 2Fe+3(aq) + Sn+2(aq) → 2Fe+2(aq) + Sn+4(aq) K = ? a. 4.04 x 107 b. 3.44 x 1018 c. 4.48...
An electrochemical cell is set up at 25°C based on the overall reaction represented by the...
An electrochemical cell is set up at 25°C based on the overall reaction represented by the balanced equation shown below. The cell initially has [Cr3+] = [Cu2+] and E°cell = +1.08 V. $$3Cu2+(aq)+2Cr(s)3Cu(s)+2Cr3+(aq) How many moles of electrons are transferred per reaction cycle (i.e., for 1 cycle of the equation as written)? 6 Part 3 (1 point) Using the relationship given in part 1, calculate Ecell if [Cu2+] = 1.453 M and [Cr3+] = 0.00176 M, assuming that the temperature remains...
Pt1 An electrochemical cell is set up at 25°C based on the overall reaction represented by...
Pt1 An electrochemical cell is set up at 25°C based on the overall reaction represented by the balanced equation shown below. The cell initially has [Cr3+] = [Cu2+] and E°cell = +1.08 V. 3Cu2+(aq)+2Cr(s)harpoon_left.pngharpoon_rigth.png3Cu(s)+2Cr3+(aq) -Using the relationship given in part 1, calculate Ecell if [Cu2+] = 1.453 M and [Cr3+] = 0.00209 M, assuming that the temperature remains at 25°C. Give your answer to two places after the decimal. (R = 8.314 J/mol·K and F = 9.65 × 104 C/mol...
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction?...
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction? (R= 8.314 J/K.mol, F = 96,500 C-moll) Sn2+ (aq) + Fe(s) Sn(s) + Fe2+(aq) E cell = 0.35 V O 7.1 x 10-11 1.2 x 1010 1.2 x 105 8.6 x 10- 2.3 1023 QUESTION 30 A chemist adds substance A and B to a reaction flask and allows equilibrium to establish A+B=CKc= 1.5 x 10-25 Which of the following describe the contents of...
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by...
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation lnK=nFE∘RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e−) , R (the gas constant) is equal to 8.314 J/(mol⋅K) , and T is the Kelvin temperature. Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 5.51×10−3.
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reacti...
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo
Question 21 of 33 What is AGº for a redox reaction where 6 moles of electrons...
Question 21 of 33 What is AGº for a redox reaction where 6 moles of electrons are transferred and E° =-4.20 V? (F = 96,500 J/(V.mol))
Question 30 (6 points) What is the equilibrium constant (K) at 25°C for the following cell...
Question 30 (6 points) What is the equilibrium constant (K) at 25°C for the following cell reaction? Sn(s) + Pb2+ (aq) → Sn2+ (aq) + Pb(s); Eºcell = 0.014 V (Please submit your detail solution work to the dropbox, which can be found in the assignments.) A/
The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by...
The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation Fe(s) + Ni+ (aq) +Fe?+ (aq) + NI(s) FE In K = Express your answer numerically. View Available Hints) where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mole). R (the gas constant) is equal to 8.314 J/(mol-K). and T is the Kelvin temperature. ΟΙ ΑΣΦ h ? KK- Submit Previous Answers *...
What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0140 V and n = 2? (F = 96,500 J/(V•mol), R = 8.314 J/ (mol·K)) 0.3353 1 2 3 x 4 5 6 с 7 00 9 O +/- x 100 Complete and balance the following redox reaction in basic solution MnO4 (aq) + C2042-(aq) → MnO2 (s) + CO2(g) 3C22 Reset < > х 1 2 3 4 5 6 7 8 9 0...
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction? (R= 8.314 J/K.mol, F = 96,500 C-moll) Sn2+ (aq) + Fe(s) Sn(s) + Fe2+(aq) E cell = 0.35 V O 7.1 x 10-11 1.2 x 1010 1.2 x 105 8.6 x 10- 2.3 1023 QUESTION 30 A chemist adds substance A and B to a reaction flask and allows equilibrium to establish A+B=CKc= 1.5 x 10-25 Which of the following describe the contents of...
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo
Question 21 of 33 What is AGº for a redox reaction where 6 moles of electrons are transferred and E° =-4.20 V? (F = 96,500 J/(V.mol))
Question 30 (6 points) What is the equilibrium constant (K) at 25°C for the following cell reaction? Sn(s) + Pb2+ (aq) → Sn2+ (aq) + Pb(s); Eºcell = 0.014 V (Please submit your detail solution work to the dropbox, which can be found in the assignments.) A/
The equilibrium constant, K. for a redox reaction is related to the standard potential, E, by the equation Fe(s) + Ni+ (aq) +Fe?+ (aq) + NI(s) FE In K = Express your answer numerically. View Available Hints) where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mole). R (the gas constant) is equal to 8.314 J/(mol-K). and T is the Kelvin temperature. ΟΙ ΑΣΦ h ? KK- Submit Previous Answers *...
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