26. Standard cell potential is measured in what specific atmospheric pressure? A. 1 atm 27. In determining the standard cell potential, what is measured between the B. 2 atm C. 3 atm D. 4 atm potentials of the two electrodes? A. Difference B. Quotient C. Product D. Sum 28. How many electrons does Au lost? Au+(aq) + Ca(s)→ Au(s) + Ca2*(aq) А. 1 В. 2 С.3 D. 4

26. Standard cell potential is measured in what specific atmospheric pressure? A. 1 atm 27. In determining the standard cell potential, what is measured between the B. 2 atm C. 3 atm D. 4 atm potentials of the two electrodes? A. Difference B. Quotient C. Product D. Sum 28. How many electrons does Au lost? Au+(aq) + Ca(s)→ Au(s) + Ca2*(aq) А. 1 В. 2 С.3 D. 4

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

What are the standard potentials for the following reactions, E°? a. Cl2(g) + 2 Br–(aq) → Br2 + 2 Cl–(aq) b. Ni(s) + 2 Fe3+(aq) → Ni2+(aq) + 2 Fe2+(aq) c. Fe(s) + 2 Fe3+(aq) → 3 Fe2+(aq)
I. Calculate the standard cell potential for each of the following reactions. 2Ag*(aq) + Pb(s) → 2Ag(s) + Pb²*{aq) a. b. 2C102(g) + 11(aq) → 2C1O2 (aq) + I2(s) O2(e) + 4H*(aq) + 2Zn(s) → 2H2O@ + 2Zn2*(aq) C.
Help me answer these 3 subunits out. Thank you!
8. Which of the following statements regarding the concentration cell are correct? I. The standard cell potential of a concentration cell changes with temperature. II. The cell potential of a concentration cell is negative if the anode electrolyte concentration is less than that in the cathode. III. The cell potential of a concentration cell is positive if the anode electrolyte concentration is less than that in the cathode. A. I only B. I and II C. II and III D. I and III E. II only F. III only
For the following voltaic cell:Fe(s) | Fe^2+(aq, 1.0 M) || Cu^2+(aq, 1.00 M) | Cu(s) a. Draw a diagram of the cell.b. Write the cell half-reactions.c. Label one half-reaction as the oxidation, the other as the reduction.
A voltaic cell consists of a Pb/Pb?+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial concentrations of Pb?+ and Cu?+ are 0.0530 mol L1 and 1.60 mol L-', respectively. Part B What is the cell potential when the concentration of Cu+ has fallen to 0.240 mol L? Pb?+ (ag) +2 e → Pb(s) E° = 0.13 V Express your answer using two decimal places. Cu (ag) + 2 e → Cu(s) E = 0.34 V Ecal = 0.489 V Submit Previous Answers Request Answer X Incorrect; Try Again Part C What are the concentrations of Pb?+ and Cu?+ when the cell potential falls to 0.36 V? Express your answers using two significant figures separated by a comma. ? [Pb* ]- [Cu*] = mol L Submit Request Answer
For the cell: Cu | Cu^2+ || Ag+ | Ag. What is the Standard Gibbs free energy? Choose the correct answer. A. 4.45x10^4 J B. -8.9x10^4 J C. 4.45x10^4 J D. 8.9x10^4 J
I. For each of the following; a. Write the overall cell reaction/ cell representation b. Calculate the standard cell potential (Eo) c. Determine whether the reaction is spontaneous or non-spontaneous. Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) Pb(s) + Sn+2(aq) → Pb+2(aq) + Sn(s) Al / Al+3 // Mg+2 / Mg Ca / Ca+2 // Cr+3 / Cr
74. A voltaic cell employs the redox reaction: Sn²+(aq) + Pb(s) Sn(s) + Pb2+(aq) E° cell = 0.010 V Calculate the cell potential, Ecell, at 25°C under each set of conditions. a. [Pb2+] = 0.010 M; [Sn²+] = 0.010 M b. [Pb2+] c. [Pb2+] = = 1.0 × 10 6 M; [Sn²+] = 2.0 M 1.5 M; [Sn2] = 0.010 M
2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
Why is the answer to this (c): If the half-cell containing 1.00 M Fe(NO3)2(aq) in galvanic cells Y and Z is replaced with a half cell containing 5.00 M Fe(NO3)2(aq), what will be the effect on the cell voltage of the two galvanic cells? a. The voltage will increase in both cells. b. The voltage will decrease in both cells. c. The voltage will increase in cell Y and decrease in cell Z. d. The voltage will decrease in cell Y and increase in cell Z.
Determine if the reaction below is spontaneous.Cl2(g) + 2 F–(aq) ⇌ F2(g) + 2 Cl–(aq)a. Based on the given reaction, write the reduction half-reaction.b. Based on the given reaction, write the oxidation half-reaction.c. By looking at the reduction potential table below, calculate the standard cell potential.