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)
The voltaic cell shown above has two identical zinc electrodes : The solution in half-cell A contains a 4.2 mol/L ZnSO4 solution. Half-cell B solution contains a 0.043 mol/L ZnSO4 solution. Calculate the emf (electromotive force) of this cell at non-standard conditions in volts (V).
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.
For each redox reaction, write the half-reactions and draw the cell diagram for a galvanic cell (use short hand cell notation) in which the overall reaction occurs spontaneously. Identify each electrode as either positive or negative. a. Ag(s) + Fe3+ (aq) → Ag+ (aq) + Fe2+ (aq)
1. Sketch an electrochemical cell that uses the given reaction. Label the anode and cathode; indicate the direction of electron flow; write a balanced equation for the cell reaction; and calculate E°cell, AG° and K. NO3^- (aq) + H^+(aq) + Zn(s) -> Zn^2+ (aq) + NO(g) + H20(l) 2. The given cell reaction is spontaneous at standard state. True or False? 3. Which is favored by the cell reaction? Reactants or Products?
|| 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
Use the hypothetical standard half-cell potentials listed below to calculate the standard cell potential in units of V for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)3 Cl 2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe 3+(aq)Cl 2(g) + 2 e⁻ → 2 Cl⁻(aq) E° = +1.73 VFe 3+(aq) + 3 e⁻ → Fe(s) E° = - 0.14 V
b) Consider a concentration cell (voltaic cell) at temperature of 25°C. The setup consists of chromium electrodes on both sides. One side is filled with 300 mL of 0.2 M chromium sulfate, Cr2(SO4)3 solution and the other side is 300 mL of 3.6 M Cr2(SO4)3 solution. i. Identify which concentration of chromate solution should be on the anode and cathode. ii. Calculate the voltage produced by the cell.
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.