From the observations listed, estimate the value of
a. The metal M reacts with
b. The metal M reacts with HCI(aq), producing
(a)
Interpretation:
The value of E°cellshould be estimated for the half reaction of
Concept introduction:
The solid metal should have higher reactivity than the aqueous metal in order to observe the displacement.
In order to react with an acid, the acid anion should have higher reduction potential while oxidizing the metal to metal cation in the acidic medium.
Answer to Problem 1E
Explanation of Solution
If M displaces the Ag+(aq) the
Therefore, lower limit of the estimation for the
(b)
Interpretation:
The value of
Concept introduction:
The solid metal should have higher reactivity than the aqueous metal in order to observe the displacement.
In order to react with an acid, the acid anion should have higher reduction potential while oxidizing the metal to metal cation in the acidic medium.
Answer to Problem 1E
Explanation of Solution
If displaces neither Zn+(aq) nor Fe2+(aq), the
Therefore, lower limit of the estimation for the
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Chapter 19 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
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- You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.arrow_forwardConsider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).arrow_forwardDescribe how to set up a voltaic cell using the following half-reactions: Reduction half-reaction:Ag+(aq) + e Ag(s) Oxidation half-reaction:Ni(s) Ni2+(aq) + 2 e Which electrode is the anode, and which is the cathode? What is the overall cell reaction? What is the direction of electron flow in an external wire connecting the two electrodes? Describe the ion flow in a salt bridge (with NaNO3) connecting the cell compartments.arrow_forward
- An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forwardAn electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 M NH3 that is also 0.010 M in Cu(NH3)42+, what is the cell potential at 25C? Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013arrow_forward
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