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Question9 Write the Nernst equation of the following cells at 298 K: (i) Mg(s) | Mg210.001...
given this electrochemical cell: Concentration of H+ is unknown, Pressure of H2 is constant at 1...
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
Which of the following is easiest to oxidize? a. H2(g) b. Zn(s) c. Ag(s) d. H2O(l)...
Which of the following is easiest to oxidize? a. H2(g) b. Zn(s) c. Ag(s) d. H2O(l) e. Cu(s) The half?reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO4 ? (aq) + 24H+ (aq) + 5Fe (s) ? 3Mn2+ (aq) + 5Fe3+ (aq) + 12H2O (l) a. MnO4 ? (aq) + 8H+ (aq) + 5e? ? Mn2+ (aq) + 4H2O (l) b. 2MnO4 ? (aq) + 12H+ (aq) + 6e? ? 2Mn2+ (aq) + 3H2O (l) c. Fe (s) ? Fe3+ (aq) + 3e? d. Fe (s) ? Fe2+ (aq) + 2e? e. Fe2+ (aq) ? Fe3+ (aq) + e can you explain in detail? I have no clue what is going...
/ Question 8 / Write a balanced net ionic equation for the overall reaction represented by...
/ Question 8 / Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag Agl|I || Fe2+, Fe3+ Pt Fe2+(ag) + Agi(s) — Fe3+(aq) + Ag(s) + F(ag) Fe?"(aq) + 21(aq) - Fe2+(aq) + 12(5) Fe3+(aq) + Ag(s) + 1-(aq) - Fe2+(aq) + AgI(s) Fe2+(aq) + Ag(s) +1-(aq) - Fe3+(aq) + AgI(s) Fe3+(ag) + Agi(s) - Fe2+(aq) + Ag(s) + (aq)
Questions I. Based on the Reduction Potential Table constructed in this experiment: For each of the...
Questions I. Based on the Reduction Potential Table constructed in this experiment: For each of the following, circle the stronger oxidizing agent: i. Ht or Fe3* ii. Cl2 or Zn2 iii. 2 or Br2 a. b. For each of the following, circle the weaker reducing agent: i. Cu or H2 ii. Br or I iii. H2 or Br Predict if he following redox rescióons will be pontaneous (S), r non- spontaneous (N): i. 2H+(aq) + 21-(aq)-- H2(g) + 12(aq) ii....
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown...
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0,...
Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equatio 1-SO3-(ag)+MnO4-(ag)+H+(ag)---->SO4^2-(ag)+Mn2+(ag)+H2O(l) 2- H2O2(ag)+ClO2(ag)+HO-(ag)---> O2(g)+ClO2-(ag)+H2O(l) Q: In the electrochemical voltaic cell using the reaction, Fe3+(aq) + Cr(s) → Fe(s) + Cr3+(aq), match the correct 1/2 reaction that occurs at the anode and cathode. 1/2 reaction occuring at the anode 1/2 Reaction occuring at the cathode Choices: A Fe3+(aq) +...
1)A voltaic cell operates at 298 K according to the following reaction: 4 Fe2+(aq) + O2...
1)A voltaic cell operates at 298 K according to the following reaction: 4 Fe2+(aq) + O2 (g) + 4 H+(aq) → 4 Fe3+ (aq) + 2 H2O (l) What is the emf of this cell when [Fe2+] = 6.5908E-4 M, [Fe3+] = 0.699 M, pressure O2 = 0.540 atm and pH = 3.10? 2)A voltaic cell operates at 298 K according to the following reaction: 3 Fe2+(aq) → Fe (s) + 2 Fe3+ (aq) What is the emf of this...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are...
A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s) K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g)...
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
please help! :( Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq...
please help! :(
Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq, 0.0010 M) || Fe3 + (aq 0.0010 M), Fe2 + (aq, 0.010 M) | Pt (s) a) Write the reaction formula for the cell b) Calculate the normal potential of the redox pair Fe3 Fe2+
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
/ Question 8 / Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag Agl|I || Fe2+, Fe3+ Pt Fe2+(ag) + Agi(s) — Fe3+(aq) + Ag(s) + F(ag) Fe?"(aq) + 21(aq) - Fe2+(aq) + 12(5) Fe3+(aq) + Ag(s) + 1-(aq) - Fe2+(aq) + AgI(s) Fe2+(aq) + Ag(s) +1-(aq) - Fe3+(aq) + AgI(s) Fe3+(ag) + Agi(s) - Fe2+(aq) + Ag(s) + (aq)
Questions I. Based on the Reduction Potential Table constructed in this experiment: For each of the following, circle the stronger oxidizing agent: i. Ht or Fe3* ii. Cl2 or Zn2 iii. 2 or Br2 a. b. For each of the following, circle the weaker reducing agent: i. Cu or H2 ii. Br or I iii. H2 or Br Predict if he following redox rescióons will be pontaneous (S), r non- spontaneous (N): i. 2H+(aq) + 21-(aq)-- H2(g) + 12(aq) ii....
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
please help! :(
Cell potential for the following cell was measured to 0.889 V at 25 ° C Pt (s) H2 (g, 0.95 bar) H(aq, 0.0010 M) || Fe3 + (aq 0.0010 M), Fe2 + (aq, 0.010 M) | Pt (s) a) Write the reaction formula for the cell b) Calculate the normal potential of the redox pair Fe3 Fe2+
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