(b)The molar conductivity (^m) of the acetic acid is given as 5.27 x 104 S m² mol-¹ at aconcentration of 100 mol m³. If the cell has a resistance of 33.01 S-1 whenfilled with 100 mol m³ KCl(aq) and 300.0 S-1 when filled with 100 mol m³CH3COOH, calculate the measured conductivity (K) of 100 mol m³ KCl(aq). Theconductivity (K) of water is 0.076 S m¹ at 25 °C.

Step 1: Step 2: Step 3: Step 4:

Answered: (b) The molar conductivity (^m) of the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 103CP

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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-.
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
Calculate the standard cell potential of the following cell at 25C. Cr(s)Cr3(aq)Hg22(aq)Hg(l)
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
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A typical total phosphate concentration in a cell, [HPO42] + [H2PO4], is 2.0 102 M. What are the concentrations of HPO42 and HPO4 at pH 7.40?
Gibbs energy change, A¡G° , is related to cell potential, Eell, by the equation A;G° = –nFEel Part B where n is the number of moles of electrons transferred Calculate the standard cell potential at 25 ° C for the reaction and F = 96 500 C mol1 is the Faraday's constant. X(s) + 2Y*(ag)→+X²+(ag) +2Y(s) where A,H° = -675 kJ mol1 and A,S° = -393 J K-1 mol-1 Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? HA Value Units %3D cell Submit Previous Answers X Incorrect; Try Again
Consider the following galvanic cell reaction at 25 oC, 4 Cr2+(aq) + O2(g) + 4 H3O+(aq) → 4 Cr3+(aq) + 6 H2O(l). Which of thefollowing statements best describes what would happen to the cell potential if the concentration of Cr2+ is increased?(a) The cell potential would become less positive.(b) The cell potential would become more positive.(c) The cell potential would remain the same.(d) It is impossible to tell.
Based on the cell notation of an electrochemical cell, Pt(s) | H2 (g, 1 atm) | H+ (aq,0.02M)|| Ag* (aq.0.15 M) Ag (s) (a) write the half-cell notation equation of the anode and cathode. (b) write the overall cell reaction equation. (c) given that the cell potential is +0.852 V, calculate the standard reduction potential of silver. (d) calculate the equilibrium constant for the reaction at 25 C.
The cell notation of an electrochemical cell is given as below. Zn(s) |Zn²*(aq, 1.0 M)|| H*(aq, 1.0 M)|H,(g, 1 atm)|Pt(s) (a) Given that the cell potential is +0.76 V at 25°C, calculate the standard electrode potential for Zn*/Zn. (b) The cell potential of the above cell is recorded as +0.67 V at 25°C when hydrochloric acid and 1.0 atm hydrogen gas is used. Calculate the pH of the hydrochloric acid.
The electromotive force of the cell Pb(s) PbSO4(s) Na2SO4.10H₂O(aq)|Hg2SO4(s) Hg() is 0.9647 V at 25 °C. The temperature coefficient is 1.74 x 10-4 V K-¹. What is the AH for the reaction in kJ mol-¹? Express your answer in four significant figures.

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