Corrosion Problem: Electrode Electrode Pb (s) PbCh (s) HCl (aqueous) AgCI (s)Ag (s) The emf of...
Pb^2+ +2e- __> Pb e=-0.13V Ag+ +1e-__> Ag e=+0.80V Pb(s)| Pb2+ (1M) || Ag+ (1M) | Ag(s) Determine which of the following statements about the cell shown are True or False. The silver half-cell is the cathode. True False The mass of the silver electrode is decreasing. True False Anions move to the silver half-cell. True False Electrons are spontaneously produced in the lead half-cell. True False The cell, as represented by the line notation, is a voltaic cell. True False The standard cell potential,...
The emf of the cell, H-(1 bar)|HCl(0.01 m)|AgClI(s)|Ag is given by E(in volts) = -0.096 + 1.90 T -3.041 x 10° T². What is the cell reaction? Calculate AG, AS, AH, and AG for the cell Eon at 298K. %3D 5. The emf of the cell, H(1 bar)|HCl(0.01 m)|AgCl(s)|Ag is given by E(in volts) = -0.096 + 1.90 x 10T-3.041 x 10-6 T2. What is the cell reaction? Calculate AG, AS, AH, and AG for the cell reaction at 298K.
all questions pleasee 2. Which of the following reactions will have the larger emfnder s ave the larger emf under standard conditions? Why? CuSO (aq)+Pb(s)PbsO ()+Cu(s) Cu(NO, ag)+P)P(NO,)a)+Cu) 3. Calculate AG for the reaction in Example 17.3. 4. Voltages listed in textbooks and handbooks are given as standard cell potentials volitas What is ceWere the cells constructed in this experiment standard cells? Why or why not? . As a standard voltaic cell runs, it "discharges" and the cell potential decreases...
help please 9.15 Consider a hydrogen electrode in HBr(aq) Estimate the change in the electro de potential when the solution is changed from 5.0 mmol dm-3 to at 25°C operating at 1.45 bar. 15.0 mmol dm3 9.16 Devise a cell in which the cell reaction is: Mn(s) + Cl2(g) MnCl2(aq). Give the half-reactions for the electrodes and from the standard cell potential of +2.54 V deduce the standard potential of the Mn2/Mn couple. 9.17 Write the cell reactions, electrode half-reactions...