Use the data below to determine which statement is true of the voltaic cell illustrated here. Fe(s) Cr(s) Salt bridge 1M Cr" 1M Fe" Fe3+ (aq) + 3e → Fe(s) E = -0.036 V Crš+ (aq) + 3e¯ → Cr(s) E = -0.73 V Cr is the anode; Fe is the cathode; electrons flow from left to right Cr is the cathode; Fe is the anode; electrons flow from left to right Cr is the anode; Fe is the cathode; electrons flow from right to left Cr is the cathode; Fe is the anode; electrons flow from right to left O O

Use the data below to determine which statement is true of the voltaic cell illustrated here. Fe(s) Cr(s) Salt bridge 1M Cr" 1M Fe" Fe3+ (aq) + 3e → Fe(s) E = -0.036 V Crš+ (aq) + 3e¯ → Cr(s) E = -0.73 V Cr is the anode; Fe is the cathode; electrons flow from left to right Cr is the cathode; Fe is the anode; electrons flow from left to right Cr is the anode; Fe is the cathode; electrons flow from right to left Cr is the cathode; Fe is the anode; electrons flow from right to left O O

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 balanced chemical reaction for the galvanic cell that contains the two half reactions. Fe3+(aq) + 3e- → Fe(s) Eo=-0.036 V Mg2+(aq) + 2e-→ Mg(s) Eo=-2.37 V what is the state of matters?
A voltaic cell prepared using zinc and iodine has the following line notation. Zn(s) | Zn2*(aq) || |'(aq) | 12(s) | C (graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction? 21 (aq) + Zn(s) → I2(s) + Zn²+(aq) 21(aq) + Zn2*(aq) → I2(s) + Zn(s) O 12(s) + Zn(s) → 21'(aq) + Zn2*(aq) 12(s) + Zn2*(aq) –→ 21(aq) + Zn(s) None of these, since graphite must be in the equation.
When nickel is placed in a copper solution, the following reaction occurs: Ni(s) + Cu2*(aq) → Ni²*(aq) + Cu(s) Select the correct cell notation for this reaction: Oa. Ni(s)|Ni2*(aq)||Cu²+(aq)|Cu(s) Ob. Ni(s) + Cu2*(aq) → Ni²*(aq) + Cu(s) Oc. Cu(s)|Cu²+(aq)||Ni²*(aq)|Ni(s) Od. Cu(s)|Ni²+(aq)||Cu²*(aq)|Ni(s) Oe. Ni(s)|Cu2*(aq)||Ni²* (aq)|Cu(s)
A voltaic electrochemical cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. → Sn²*(aq) + Hg(1) 2+, Sn(s) + Hg²*(aq) · What is the reaction that takes place in the anode compartment? + + What is the reaction that takes place in the cathode compartment? + + In the external circuit, electrons migrate v the Hg²* electrode v the Sn electrode. In the salt bridge, anions migrate the Hg** compartment| v the Sn compartment.
|| Cu²+ Cu . What half reaction is Consider the cell Zn| Zn² taking place at the anode? Zn2+ Zn(s) → Zn²+ (aq) + 2e Cu 2+ (aq) → Cu(s) + 2e Cu(s) → Cu 2+ (aq) + 2e Zn 2+ (aq) → Zn(s) Zn(s) + 2e
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb+2 half cell. All solutions are 1.0 M. Ag+(aq) + e- → Ag(s) E° = 0.80 V Pb+2(aq) + 2e- → Pb(s) E° = -0.13 V a.Diagram the cell, labeling electrodes and solutions, show the direction of electron flow in the circuit and what occurs in the salt bridge. b. If the cell were made with [Pb+2] = 0.10 M and [Ag3+] = 3.0 M, would the voltage increase, decrease, or remain the same? Explain using Q. c.Identify the electrode that is gaining mass
O ELECTROCHEMISTRY Analyzing a galvanic cell A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2 Cr(OH)3(s) + 10OH (aq) - → 6 Br (aq) + 2 CrO (aq) + 8 H₂0(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 E = OV ローロ é X Do ?
The following oxidation-reduction reactions are used in electrochemical cells. Write them using cell notation. a) Write the net equation for the redox reaction that occurs in the voltaic cell: Sc(s) │Sc3+(aq) ║ Ag+(aq) │Ag(s) (Hint: Assume that the customary conventions were used in writing the cell diagram.) b) Draw a voltaic cell in which the displacement of silver ions from solution by aluminum metal occurs. Label the cathode, the electrons. Also, indicate the direction of the flow of cations and anions from the KNO3 (aq) salt bridge. Write an equation for the half-reaction occurring at each electrode, write a balanced equation for the overall reaction, and write the cell diagram.
Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
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