What is the emf of a cell consisting of a Pb²* / Pb half-cell and a Pt/H* / H₂ half-cell if [Pb²+]=0.50 M, [H] = answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional Information. =0.027 M and PH₂ =1.0 atm? Round your

What is the emf of a cell consisting of a Pb²* / Pb half-cell and a Pt/H* / H₂ half-cell if [Pb²+]=0.50 M, [H] = answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional Information. =0.027 M and PH₂ =1.0 atm? Round your

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What is the standard cell potential for the reaction below? Enter your answer with two decimal places and no units. Mg(s) + Br2() Mg2+(aq) + 2 Br"aq) The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Bro/Br half-cell. Enter your answer in decimal format using two decimal places, (value + 2%).
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
A voltaic cell consists of an Al/Al3+ half-cell and a Fe2+/Fe3+ half-cell. The standard reduction potential for Al3+ is −1.66V and for Fe3+ is 0.77 V. Calculate Ecell at 25 ºC when the concentration of [Al3+] = 9.51 x 10-4 M , [Fe3+]= 6.24 x 10-3 M, and [Fe2+]= 5.74 x 10-5 M
half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V red MnO, (aq)+2 H,0(1)+3e MnO,(5)+4 OH (aq) E° =+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If said it was you possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…
The Nernst Equation A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E = E° - where E = potential under nonstandard conditions %3D E = standard potential R = ideal gas constant = 8.314 J/K mol %3D T = kelvin temperature n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons = %3D 96, 485 C/mol = 96, 485 J/V mol %3D Q = reaction quotient %3D It is customary to use the equation in a form where numberical values are substituted for R, T, and F at a temperature of 25°C. (8.314 J/K mol)(298K) 96, 485 J/V mol RT = 0.02568 V %3D and the Nernst equation with the potentials in volts is: 0.02568 In Q E = E - n Sometimes it is more convenient to use base-10 logarithms, and the substitution of 2.3026 log for In is made. (2.3026 x 0.02568 = 0.0591) %3D 0.0591 logQ E = E° – A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Use…
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V
A Galvanic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V). Calculate [Au3+] in molar concentration if [Cu2+] = 1.00 M and Ecell = 1.13 V at 25°C. Keep 2 decimals.
Predict reaction and calculate E°cell from standard reduction potentials. A voltaic cell is constructed from a standard AI3+|Al half cell (E°red = -1.660V) and a standard F2|F° half cell (E°red = 2.870V). What is the spontaneous reaction that takes place, and what is the standard cell potential? Spontaneous cell reaction:Write a balanced equation using the smallest integer coefficients possible. + Standard cell potential: V.
At a temperature of 25 ° C the galvanic element Pt | MnO4- 0,10M, Mn2 + 0,1M, pH = 1 | Ag + 0.0001M | Ag has the electromotive force 0,80V. Calculate the standard electrode potential of Ag + if E ° (MnO4 -, H + | Mn2 +) = 1.50V
Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25.0 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)