Calculate the initial AgNO 3 electrolyte concentration in thecathode half-cell for the concentration cell shown belowimmediately after it has just been assembled at 25 °C. Theinitial standard cell potential is measured to be Ecell = +0.038V.SilverElectrodeVSilverElectrodeAg*Ag*NO3NO30.01 M AgNO3? M AgNO3a. 3.30 x 104 Mb.8.60 × 10 3 MC. 0.010 Md.0.060 Me. 0.300 M

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Answered: Calculate the initial AgNO 3…

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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Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol
Consider the following cell reaction: Mn(s) + 2 H*(? M) Mn²*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.322 volts, what is the pH of the hydrogen electrode? pH
Consider an electrochemical cell made up of Au Au* and Co²+ | Co³+ half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E = ローロ V 00 Calculate the standard emf of a cell that uses the Au Au and Co²+ | Co³+ half-cell reaction at 25 °C. Round your answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. 09 S
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
3. For the reaction: Zn(s) + 2Ag+ (aq) → Zn+2(aq) 2Ag(s). a. Determine the standard cell potential. b. Is the reaction spontaneous? If yes, write the cell notation.
2+ Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² ]=0.761 Mand [Ni²+]=0.0180 M. Use the standard reduction potentials from the 2+ appendix in the book. 2+ ↔ Mg²+ (aq) + Ni(s) Give the numeric value only assuming a measurement in V Mg(s) + Ni²+ (aq) → 2+ (aq)
The anode compartment of a galvanic cell consists of a Zn anode immersed in 0.05M ZnCl2 The cathode compartment consists of a Cu cathode immersed in an 0.10M CuCl2 solution. Using the cell potentials found on page 815 of your textbook, calculate the cell potential for this reaction. Assume T = 298K.
The free energy change for the following reaction at 25 °C, when [Hg²+] = 1.20 M and [Pb2+] = 7.55x10-3 M, is -202 kJ: Hg2+(1.20 M) + Pb(s) Hg(l) + Pb2+(7.55×10-3 M) AG = -202 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction? forward or reverse
If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode
Consider the electrolysis reactions cathode anode whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = Cu²+ (aq, 0.177 M) +2e=Cu(s) H₂O(1) ⇒ 10₂(g, 1 bar) + 2 H+ (aq, 0.195 M) + 2 e¯ The cell has a resistance of 66.0 and a current of 7.17 mA when the cathode overpotential is 0.231 V and the anode overpotential is 0.050 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Ecell = V V
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
What is the calculated value of the cell potential at 298 K for an 2+ Cu²+ concentration is 3.83 × 10-4 M and the A1³+ concentration is 1.12 M? Ecell electrochemical cell with the following reaction, when the 2+ 3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq) V The cell reaction as written above spontaneous nonspontaneous for the concentrations given.

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