When EoAg+/Ag = 0.8 V and EoZn2+/Zn = −0.76 V, which of the following is correct (Hint: standard reduction potentials are measured with reference to S.H. E)
a. Ag+ can be reduced by H2
b. Ag can oxidize H2 into H+
c. Zn2+ can be reduced by H2
d. Ag can reduce Zn2+ ion
When EoAg+/Ag = 0.8 V and EoZn2+/Zn = −0.76 V, which of the following is correct...
Given the following half-cell potentials, i. Zn2+ + 2 e– → Zn (E° = –0.76 V) ii. Cr3+ + 3 e– → Cr (E° = –0.74 V) determine the cell potential whose overall redox reaction under standard conditions is 3 Zn(s) + 2 Cr3+(aq) → 3 Zn2+(aq) + 2 Cr(s): * A. –0.80 V B. –0.02 V C. +0.02 V D. +0.80 V
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An electrochemical reaction occurring in a galvanic cell is expressed using the standard cell notation: Zn(s) Zn2+ (aq) || Ag (aq) | Ag(s) The standard reduction potentials for the half-cell reactions are as follows: Zn2+(aq) + 2e_? Zn(s) E o=-0.76 V Ag (a)eAg(s) E +0.80 V Which of the following statements is correct regarding this electrochemical cell? A. Agt is reduced at the cathode; Zn is oxidized at the anode. B. Edell = +1.56 V...
A battery is constructed at 25ºC using the voltaic cell with initial concentrations Zn│Zn2+ (0.100 M) ││Ag+ (1.500 M) │Ag How much does the cell voltage drop when 95% of the capacity (i.e., the concentration of Ag+ drops to 5% of its starting value) is consumed? The standard reduction potentials for the two half-cells are + Zn2+ + 2e- → Zn Eº = − 0.76 V Ag+ + e- → Ag Eº = 0.80 V
A battery is constructed at 25ºC using the voltaic cell with initial concentrations Zn│Zn2+ (0.100 M) ││Ag+ (1.500 M) │Ag How much does the cell voltage drop when 95% of the capacity (i.e., the concentration of Ag+ drops to 5% of its starting value) is consumed? The standard reduction potentials for the two half-cells are Zn2+ + 2e- → Zn Eº = − 0.76 V Ag+ + e- → Ag Eº = 0.80 V
Question 7 (1 point) Saved Consider these metal ion/metal standard reduction potentials Cu2(aq)|Cu(s) Ag+1(aq)|Ag(s) Co2(aq)|Co(s) Zn+2(aq)]Zn(s) +0.34 +0.80 V -0.28 V -0.76 V Based on the data above, which one of the species below is the best oxidizing agent? 0 1 Cols) O2) Zn(s) 3) Cutlaq) 04) Culs) 5) Ag+h(aq)
Standard reduction potentials for the Zn2+/Zn and Pb2+/Pb couples are -0.76 and - 0.13 V, respectively. The galvanic cell below uses the half-cells Pb2+ Pb and Zn2+|Zn, and a salt bridge containing KCl(aq). The voltmeter gives a positive voltage reading. voltmeter salt bridge CD- <-CD-RB B The electrode B could be inert platinum metal or lead metal. O True O False
Question 7 (1 point) Standard reduction potentials for the Zn2+/Zn and Pb2+/Pb couples are -0.76 and - 0.13 V, respectively. The galvanic cell below uses the half-cells Pb2+[Pb and Zn2+|Zn, and a salt bridge containing KCl(aq). The voltmeter gives a positive voltage reading. voltmeter salt bridge CD-> The identities of B and D, respectively, are O Pb and Cl- Ozn and Cl- O Pb and K+ O Zn and K+
What is the potential of the cell involving this reaction? Zn + 2Ag+ → Zn2+ + 2Ag Reaction Standard Reduction Potential Zn2+ + 2e– → Zn E0 = –0.76 V Ag+ + e– → Ag E0 = +0.80 V Question options: a. 0.84 V b. 0.04 V c. 2.36 V d. 1.56 V
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
Chemistry:
Experimental Cell Potential Lab report
please help checking my work and answering question #2 #3
#4
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*question #2 #3 #4*
Note that the ionic form of Ag is Ag' and of Fe is Fe Write a chemical reaction for each cell. For the reactants, choose the metal that was oxidized ion that was reduced spontaneously (i.e, a + potential) according to your data. (Thesethe elements!) Chemical reaction (oall) Cell notation (see text) (NA1 Zn(s)+Cu-Zn+Cu(s) r凸の, Zn(s) | Zn2...