Calculate E, E, and AG for the following cell reaction: 3Zn(s) + 2Cr (ag) = 3Zn (ag) + 2 Cr (s) where [cr**]-00 Zn*=0.0095 M. Round each of your answers to 2 significant digits. 0.040 M and Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 x 10 V• mol

Calculate E, E, and AG for the following cell reaction: 3Zn(s) + 2Cr (ag) = 3Zn (ag) + 2 Cr (s) where [cr**]-00 Zn*=0.0095 M. Round each of your answers to 2 significant digits. 0.040 M and Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 x 10 V• mol

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...

See similar textbooks

Similar questions

1. A concentration cell is constructed using two metal (M) electrodes with M 2+ concentrations of 0.10 M and 1.00 × 10 –5 M in the two half-cells. Determine the reduction potential of M 2+ given that the potential of the cell at 25°C is 0.118 V.a. 0 Vb. +0.118 Vc. –0.118 Vd. Cannot be determined with the information given.e. None of the above.
Calculate Eº, E, and AG for the following cell reaction: 2+ Mg(s) + Sn²+ (aq) ⇒ Mg²+ (aq) + Sn (s) where [Mg²+] = 0.040 M and [Sn²+] = 0.060 M. Round each of your answers to 4 significant digits. 2+ 2+ Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10ª J V.mol
A standard galvanic cell is constructed in which a Co2+ | Co half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) The cathode reaction is Co2+ + 2e -> Co. Co is oxidized at the cathode. The anode compartment could be Fe³+|Fe²+. As the cell runs, anions will migrate from the Co²+ | Co compartment to the other compartment. In the external circuit, electrons flow from the Co²+ | Co compartment to the other compartment.
4. The cell diagram for an electrochemical cell is given below: Mn(s) | Mn* (aq, 1.0 mol dm) || Ag* (aq, 1.0 mol dm)|Ag (s) In the above cell, the standard electrode potential of the silver hal f-cell is =0.80 V. E°cell = +1.98 V Write the equation for the reaction occurring at the anode and cathode. Write the overall cell equation Determine the standard electrode potential of the Mn2*/Mn half-cell What is the strongest oxidizing agent in the above cell? What is the strongest reducing agent in the above cell? a) 1) ii) b) i) i1) c) After the cell was used, the change in mass of the silver electrode was found to be 5.40 IS g Caleulate the change in mass of the manganese electrode.
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!
Calculate Eº, E, and AG for the following cell reaction: 2+ 2+ Mg(s) + Sn²+ (aq) = Mg²+ (aq) + Sn (s) 2+ 2 where [Mg²+] = [Mg²+] = 0.040 M and [Sn²+] = 0.030 M. Round each of your answers to 4 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. Note: The Faraday constant is 9.649 × 10ª Part: 0 / 3 Part 1 of 3 Eº = v V x10 J V. mol S I
Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous
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.
Calculate the Ecell Value at 298 K for the cell based on the reaction: Cu(s)+2Ag*(aq) Cu²+(aq) +2Ag(s) where [Ag*] = 0.00375 M and [Cu2+] = 8.25×104 M. The standard reduction potentials are shown below: Ag"(aq) +e → Ag(s) E° : 0.7996 V Cu²+ (aq) + 2e¯ → Cu(s) E° = 0.3419 V 3rd attempt Feedback Ecell= 0.47713 V
please answer all as they are part of 1 question but different questions,,.
Give typed explanation not a single word hand written otherwise leave it the answer is 0.03295 please help me understand how that is the answer
Calculate £º, E, and ▲g for the following cell reaction: 3+ 3Zn(s) + 2 Cr³+ (aq) = 3Zn²+ (aq) + 2 Cr (s) where [c₁³+]=0.090 M and [Zn²+] = 0.0055 M. Round each of digits. Note: Reference the Standard reduction potential nformation. J Note: The Faraday constant is 9.649 × 104. V.mol