(a) Explain why the cell emf is independent of the physical size of the cell.(b) What is the significance of the standard hydrogen electrode?

(a) cell emf independent of the physical size of the cell. An electrochemical cell is a device which…

Answered: (a) Explain why the cell emf is…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 50QRT

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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-.
(a) How many minutes does it take to form 10.0 L of O₂ measured at 99.8 kPa and 28°C from water if a current of 1.3 A passes through the electrolytic cell? (b) What mass of H₂ forms?
(b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a period of 20 min, the cathode increased weight by 2.628g. What was the current in amperes used?
A fuel cell develops an electric potential from the chemical reaction between reagents supplied from an outside source. What is the potential of a cell fuelled by (a) hydrogen and oxygen, (b) the complete oxidation of benzene at 10 bar and 298 K?
(b) The electrolysis of a solution of sodium nitrate, NaNO3, 1.0 M is carried out by using carbon electrodes anode and cathode. i) Calculate the volume of gas evolved at anode (at s.t.p) when a current of 2.50 A was passed through the solution for 45 minutes.
State what you would expect to happen to the cell potential when the following changes are made to the corresponding cells devised as attached. Confirm your prediction by using the Nernst equation in each case.(a) The molar concentration of FeSO4 is increased.(b) Some nitric acid is added to both cell compartments.(c) The pressure of oxygen is increased.(d) The pressure of hydrogen is increased.(e) Some (i) hydrochloric acid. (ii) hydroiodic acid is added to both compartments.(f) Hydrochloric acid is added to both compartments.
For the standard cell potentials given here, determine the ΔG° for the cell in kJ.(a) 0.000 V, n = 2(b) +0.434 V, n = 2(c) −2.439 V, n = 1
A current of 8.46×104 A is passed through an electrolysis cell containing molten KCl for 10.3 days.(a) How many grams of potassium are produced? g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm?
Express the relation among the cell constant, the resistance of the solutionin the cell and the conductivity of the solution. How is molar conductivity of a solution related to its conductivity?
A current of 7.14×104 A is passed through an electrolysis cell containing molten KCl for 13.9 days.(a) How many grams of potassium are produced? g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L
What do you mean by ( i) negative standard electrode potential and(ii) positive standard electrode potential ?
. (a) Balance the following simple redox reaction.Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4 OH- (3)(b) If the standard change in the Gibbs energy of the molar reaction in part (a) is-507.13 kJ. Calculate the cell potential of the reaction.

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(a) Explain why the cell emf is independent of the physical size of the cell. (b) What is the significance of the standard hydrogen electrode?