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selected answer is incorrect Question 8 0 / 1 point Calculate the equilibrium constant, K, for...
selected answer is incorrect please solve Question 8 0 / 1 point Calculate the equilibrium constant, K, for the spontaneous galvanic cell between Pb2+/Pb and Cr3+/Cr2+ conducted at standard conditions. 7.9 x102 1.7 x1014 3.1 x109 5.6 x104
Question 8 (1 point) Calculate the equilibrium constant, K, for the spontaneous galvanic cell between Pb2+/Pb and Cr3+/Cr2+ conducted at standard conditions. 7.9 x102 1.7 x1014 3.1 x109 5.6 x104 Show Report OE PASSW STRAIN605 lenovo
Calculate the equilibrium constant, K, at 298 K for the cell: Pb |Pb2+ || Ag+ | Ag The standard reduction potential for the Pb2+/Pb couple is -0.13 V, and it is +0.80 V for the Ag+/Ag couple.
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
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
6) Calculate the equilibrium constant K at 25°C for the following reaction for tant K at 25°C for the following reaction for the standard cell potential (7 points) (nFEⓇ - RT In K, F=96485 C/mol.R=8.31 J/molk) Pb2+ (aq) + Fe(s) 5 Pb(8) + Fe²(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() Ecell - Eºcell = 0.0592/n logQ
A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: 2Fe3+(aq) + Pb(s) ---> 2Fe2+(aq) + Pb2+(aq) Answer: ____ kJ K for this reaction would be ________ (greater/less) than one. B) The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.12 M and [H+] = 6.80×10-3 M, is -178 kJ: Hg2+(1.12 M) + H2(g) ---> Hg(l) + 2H+(6.80×10-3 M) ΔG =...
Please answer BOTH parts to this question. Thanks (1) The equilibrium constant of the reaction 2 C3H6(g) C2H4(g) + C4H8(g) is found to fit the expression In K= A + B/T + C/T2 between 300 K and 600 K, with A = -1.04, B = -1088 K, and C = 1.51 10% K2. Calculate the standard reaction enthalpy at 400 K. (2) Consider the electrochemical cell Ag|AgBr(s)|KBr(aq,0.050 molal)||Cd(NO3)2 (aq,0.010 molal)|Cd. Calculate the cell potential.
A student made measurements on some electrochemical cells and calculated three quantities 0 The standard reaction free energy AG . The equilibrium constant K at 25.0 °C 0 The cell potential under standard conditions E. His results are listed below Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any Note: If there is a mistake in a row, only one of the three...
Help! Not sure how to answer this whole question O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free energ... A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG'. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in...