Question 1 In the balanced cell reac Mg Mg(NO₂), The standard (assuming Voltmeter Given the electrochemical cell in the picture: V salt bridge The silver electrode gains mass be Ag ([Select] from the Ag electrode to the Mg electrode through the wire The electrons would flow from the Mg electrode to the Ag electrode through the wire from the Ag electrode to the Mg electrode through the salt bridge from the Mg electrode to the Ag electrode through the salt bridge AgNO, The change in standard Gibbs' Energy, AG, for the overall reaction would be 609 kJ/mol If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] -0.0100 M, the cell potential would then be [Select]

Question 1 In the balanced cell reac Mg Mg(NO₂), The standard (assuming Voltmeter Given the electrochemical cell in the picture: V salt bridge The silver electrode gains mass be Ag ([Select] from the Ag electrode to the Mg electrode through the wire The electrons would flow from the Mg electrode to the Ag electrode through the wire from the Ag electrode to the Mg electrode through the salt bridge from the Mg electrode to the Ag electrode through the salt bridge AgNO, The change in standard Gibbs' Energy, AG, for the overall reaction would be 609 kJ/mol If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take If the concentrations were changed to [Mg2+] = 5.00 M and [Ag*] -0.0100 M, the cell potential would then be [Select]

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter32: Voltaic Cell Measurements

Section: Chapter Questions

Problem 2ASA

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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, .
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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
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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.
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Consider a voltaic cell at 25°C in which the following reaction takes place: MnO2(s)+4H+(aq)+2Br(aq)Br2(l)+Mn2+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Find E under the following conditions: [Mn2+]=0.60M,[Br]=0.83M,pH=3.71 .