(a)
Interpretation:
The electrode potentials of the HCl (1.53 M) | H2 (0.929 atm), Pt half-cell should be determined.
Concept Introduction :
Nernst equation gives the cell potential under non-standard conditions.
E − cell potential
E0 − standard cell potential
R − universal gas constant
T − temperature in Kelvin
n − number of electrons transferred
F − Faraday constant
Q − reaction quotient
(b)
Interpretation:
The electrode potentials of the IO3- (0.154 M), I2 (2
Concept Introduction :
Nernst equation gives the cell potential under non-standard conditions.
E − cell potential
E0 − standard cell potential
R − universal gas constant
T − temperature in Kelvin
n − number of electrons transferred
F − Faraday constant
Q − reaction quotient
(c)
Interpretation:
The electrode potentials of the Ag2CrO4 (sat’d), CrO42- (0.0625 M) | Ag half-cell should be determined.
Concept Introduction :
Nernst equation gives the cell potential under non-standard conditions.
E − cell potential
E0 − standard cell potential
R − universal gas constant
T − temperature in Kelvin
n − number of electrons transferred
F − Faraday constant
Q − reaction quotient
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Chapter 22 Solutions
Principles of Instrumental Analysis
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- For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+arrow_forwarda Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).arrow_forwardThe 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.arrow_forward
- For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?arrow_forward
- What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)arrow_forwardGalvanic 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?arrow_forwardThe cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?arrow_forward
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