Answered: What would the potential of a standard…

What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+] = 0.76 M PH₂ = 4.3 atm E = T = 298 K

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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4) So far, we have looked at finding cell potentials under standard conditions, however in reality, we are seldom at standard conditions. Recall that our equation for the Gibbs free energy at nonstandard conditions was AG=AG+RTINQ By substituting -nFE for G in the above equation we come to the Nernst equation (shown below), which gives a way to predict E under any conditions, not just standard conditions. In this equation, R is the gas constant (8.314 J mol K). F is the Faraday Constant (96480 C mol) and Q is the reaction quotient. RT E=E no cell The Nemst equation is extremely powerful, and can be written in a slightly more useful form. First, the natural log (In) can be replaced by log base 10 (log) by multiplying by 2.3 (InQ = 2.3logQ), and we can rearrange terms to put the equation into the form of a straight line, as shown. El 2.3RT nFlogQ+ Ecell a) Consider this form of the Nernst equation, sketch a plot of E. vs logQ. b) Notice that the term "-(2.3*RT/nF)" is made up entirely of…
[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? [H+] = 0.72 M PH₂ = 2.7 atm E = T = 298 K V
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the [M3*], in moles per liter, required to generate a cell potential (Ecell) of 0.584 V for this reaction at 58.1 °C when [N*] = 1.246 M? Enter your answer to the thousandths place. Do not include units. M(s) + 3N*(aq) –→ M3+(aq) + 3N(s) E°cell = 0.572 V
Calculate the cell potential of each of the following electrochemical cell at 25oC. a. Pt|H 2 (8.00 atm)|H + (1.00 x 10 -3 M)‖Ag + (0.00549 M)|Agb. Pt|H 2 (1.00 atm)| H + (pH = 5.97 ) ‖ H + (pH=3.47)|H 2 (1.00 atm)|Ptc. Pt|H 2 (0.0361 atm)|H + (0.0175 M)‖H + (0.0175 M)|H 2 (5.98 x 10 -4 atm)|Pt Please solve and give explanations steps.
1- In preparing the burette for titration the final rinse should be done by: a) NaOH solution b) Titrant c) Analyte d) Deionised water 2 - The evidence of the reaction between NH. Cla and NaOH (ag) is: a) Temperature decreasedb) Color change d) Change in odor c) Precipitate appear 3 - Aspirin is produced by the reaction of aceticanhydride with: a) Acetylsalicylic acid b) Acetic acid c) Sulfuric acid d) Salicylic neid 4 - If 10ml of KOHlag was used to titrate 15ml of 0.1M KHP solution the molar concentration ofKOH solution is: a) 1.5M b) 0.15M c) 15*10^-3 M d) 0.67M
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the cell potential (Ecell), in volts, for this reaction at 35.4 °C when [M+] = 0.00533 M and [N2+] = 0.725 M? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) E°cell = 0.128 V
For the cell below, the standard potential is Eocell = 1.62 V ( F =96500 C/mole e-)( 1VC=1J) Mg(s) | Mg2+ (1M) || Zn 2+ (1M) | Zn (s)Calculate ΔGo for the cell at standard conditions in kJ. Select one: a. -1.62 kJ b. -313 kJ c. -3.13 x 105 kJ d. -156 kJ
Part A The following galvanic cell has a potential of 1.214 V at 25 °C: Hg(1)|Hg₂Br₂ (s)|Br¯(0.10 M)||MnO4¯ (0.10 M), Mn²+ (0.10 M), H+(0.10 M)|Pt(s) Calculate the value of Ksp for Hg₂Br₂ at 25 °C. Express your answer using one significant figure. Ksp = Submit 17 ΑΣΦ Request Answer ?
Calculate the potential for each cell as written at 25 °C. Indicate whether the metal electrode in the half-reaction opposite the standard hydrogen electrode, S.H.E., would be the anode or the cathode if the cell was shorted and electrons were allowed to flow freely. S.H.E. || Zn²+ (aq, 0.0110 M)| Zn(s) Ecell = Pt(s) | V3+ (aq, 0.450 M), V²+ (aq, 0.00420 M) || S.H.E. Ecell = EZn²+ Zn Incorrect = -0.762 V V V E√3+√√²+ = -0.255 V