Please help with these ZnThe electrons would flowZnSO4+salt bridgeCuIf the cell pictured above is driven as an electrolytic cell:CuSO4The following statement is true:from the Cu anode to the Zn VThe standard (assuming 1 M concentrations) cell potential is-1.10 V[Select][Select]The anions travel toward the anode which is the negative terminalIf the salt bridge contains KCI, th The anions travel toward the cathode which is the positive terminalThe anions travel toward the anode which is the positive terminalThe anions travel toward the cathode which is the negative terminalSelectIn order to decrease (make it a smaller number) the potential necessary for electrolysis,If the current is set to a constant of 3.82 A for 5.00 min. then 0.389 gof metal would deposit on the cathode. salt bridgeZnCuIZnSO4CuSO4The electrons would flowVORMING SUELIf the cell pictured above is driven as an electrolytic cell:The standard (assuming 1+The following statement is true:from the Cu anode to the Zn ✓[Select]from the Cu anode to the Zn cathodefrom the Zn cathode to the Cu anode-1.10 Vfrom the Zn anode to the Cu cathodefrom the Cu cathode to the Zn anode[Select]If the salt bridge contains KCI, then [Select]In order to decrease (make it a smaller number) the potential necessary for electrolysis.If the current is set to a constant of 3.82 A for 5.00 min. then0.389 gSelectof metal would deposit on the cathode.

We have to identify which option is correct among the given.

Zn The electrons would flow ZnSO4 I + salt bridge If the cell pictured above is driven as an electrolytic cell: CuSO4 from the Cu anode to the Zn V The following statement is true: The standard (assuming 1 M concentrations) cell potential is -1.10 V [Select] [Select] The anions travel toward the anode which is the negative terminal If the salt bridge contains KCI, th The anions travel toward the cathode which is the positive terminal The anions travel toward the anode which is the positive terminal The anions travel toward the cathode which is the negative terminal Track Serecur

Zn The electrons would flow ZnSO4 I + salt bridge If the cell pictured above is driven as an electrolytic cell: CuSO4 from the Cu anode to the Zn V The following statement is true: The standard (assuming 1 M concentrations) cell potential is -1.10 V [Select] [Select] The anions travel toward the anode which is the negative terminal If the salt bridge contains KCI, th The anions travel toward the cathode which is the positive terminal The anions travel toward the anode which is the positive terminal The anions travel toward the cathode which is the negative terminal Track Serecur

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

See similar textbooks

Similar questions

Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider the concentration cell shown below. Calculate the cell potential at 25C when the concentration of Ag+ in the compartment on the right is the following. a. 1.0 M b. 2.0 M c. 0.10 M d. 4.0 105 M e. Calculate the potential when both solutions are 0.10 M in Ag+. For each case, also identify the cathode, the anode, and the direction in which electrons flow.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
A galvanic cell is based on the following half-reactions at 25C: Ag++eAg H2O2+2H++2e2H2O Predict whether is larger or smaller than for the following cases. a. [Ag+]=1.0M,[H2O2]=2.0M,[H+]=2.0M b. [Ag+]=2.0M,[H2O2]=1.0M,[H+]=1.0107M
The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?