C) Calculate the value of Ece for this system at equilibrium. Number cell D) Determine the pH at which the given concentrations of Pb2,Pb Mn2, and MnO would be at equilibrium. Number pH
Homework Answers
> To find Ecell you do:
0.183-(0.0591/10)xlog((Pb2+)^5 x (MnO4-)^2 x (H+)^16 / (Mn2+)^2 x (PB4+)^5) like shown above but that's it. You don't subtract anything.
To find the pH you do:
Your K=(Pb2+)^5 x (MnO4-)^2 x (H+)^16 / (Mn2+)^2 x (PB4+)^5)
and then negative log that value to find pH.
mochi12 Mon, Dec 6, 2021 5:36 PM
Add Answer to:
A solution containing the following was prepared: 0.15 M Pb2. 1.5% 10.6 M Pb4t, 1.5x 106 M Mn2. 0.15 M MnO4, and 0.88 M HNO3. For this solution, the following balanced reduction half-reactions and o...
A solution containing 0.190.19 M Pb2+Pb2+ , 1.5×10−61.5×10−6 M Pb4+Pb4+ , 1.5×10−61.5×10−6 M Mn2+Mn2+ , 0.190.19...
A solution containing 0.190.19 M Pb2+Pb2+ , 1.5×10−61.5×10−6 M Pb4+Pb4+ , 1.5×10−61.5×10−6 M Mn2+Mn2+ , 0.190.19 M MnO−4MnO4− , and 0.900.90 M HNO3HNO3 was prepared. For this solution, the balanced reduction half‑reactions and overall net reaction shown can occur. 5[Pb4++2e−↽−−⇀Pb2+]5[Pb4++2e−↽−−⇀Pb2+] ?∘+=1.690 VE+°=1.690 V 2[MnO−4+8H++5e−↽−−⇀Mn2++4H2O]2[MnO4−+8H++5e−↽−−⇀Mn2++4H2O] ?∘−=1.507 VE−°=1.507 V 5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO−4+16H+5Pb4++2Mn2++8H2O↽−−⇀5Pb2++2MnO4−+16H+ A. Determine ?∘cellEcell∘, Δ?∘ΔG∘, and ?K for this reaction. ?∘cell=Ecell∘= V Δ?∘=ΔG∘= J ?=K= B. Calculate the value for the cell potential, ?cellEcell, and the free energy, Δ?ΔG, for the given conditions....
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I need help with just the last part where it asks to find the
pH.
A solution containing 0.1 7 M Pb". 1.5 x 10-6 М РЬ". 1.5 x 10-6 M Mn". 0.17 M MnO-, and 0.88 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. E1.690Vv E1.507 V A. Determine E AG, and K for this reaction. Eel0.183 AG-176600 9.024 x1030 B. Calculate the value for the cell potential, Ecell,...
For the reaction below, find answers for the following 3 questions. In acidic solution, O, and...
For the reaction below, find answers for the following 3 questions. In acidic solution, O, and Mn2 ions react spontaneously 0;(&) + Mnaq) + H2O(1) 0.8) + MnO (3) + 2H+ (aq) -0.84 V 1. Calculate in Vand enter to 2 decimal places. 2. Calculate AG (kJ/mole) for the reaction shown above and enter to 1 decimal place 3. Calculate Kat 298 K Enter e notation for large or small numbers.eg, enter 6.7e-34 for 6.7*10% 6.7e34 for 6.7*10% Enter a...
Using the standard reduction potentials listed, calculate the equilibrium constant for each of the following reactions...
Using the standard reduction potentials listed, calculate the
equilibrium constant for each of the following reactions at 298
K.
A) Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)
Express your answer using two significant figures.
B) Co(s)+2H+(aq)→Co2+(aq)+H2(g)
Express your answer using two significant figures.
C) 10Br−(aq)+2MnO−4(aq)+16H+(aq)→2Mn2+(aq)+8H2O(l)+5Br2(l)
Express your answer using two significant figure.
E°(V) -0.83 +0.88 +1.78 +0.79 Half-Reaction E°(V) Half-Reaction Ag+ (aq) + - Ag(s) +0.80 2 H20(1) + 2 e — H2(8) + 2 OH+ (aq) AgBr(s) + - Ag(s) + Br" (aq) +0.10 HO2...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
I need help with just the last part where it asks to find the
pH.
A solution containing 0.1 7 M Pb". 1.5 x 10-6 М РЬ". 1.5 x 10-6 M Mn". 0.17 M MnO-, and 0.88 M HNO, was prepared. For this solution, the balanced reduction half-reactions and overall net reaction shown can occur. E1.690Vv E1.507 V A. Determine E AG, and K for this reaction. Eel0.183 AG-176600 9.024 x1030 B. Calculate the value for the cell potential, Ecell,...
For the reaction below, find answers for the following 3 questions. In acidic solution, O, and Mn2 ions react spontaneously 0;(&) + Mnaq) + H2O(1) 0.8) + MnO (3) + 2H+ (aq) -0.84 V 1. Calculate in Vand enter to 2 decimal places. 2. Calculate AG (kJ/mole) for the reaction shown above and enter to 1 decimal place 3. Calculate Kat 298 K Enter e notation for large or small numbers.eg, enter 6.7e-34 for 6.7*10% 6.7e34 for 6.7*10% Enter a...
Using the standard reduction potentials listed, calculate the
equilibrium constant for each of the following reactions at 298
K.
A) Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)
Express your answer using two significant figures.
B) Co(s)+2H+(aq)→Co2+(aq)+H2(g)
Express your answer using two significant figures.
C) 10Br−(aq)+2MnO−4(aq)+16H+(aq)→2Mn2+(aq)+8H2O(l)+5Br2(l)
Express your answer using two significant figure.
E°(V) -0.83 +0.88 +1.78 +0.79 Half-Reaction E°(V) Half-Reaction Ag+ (aq) + - Ag(s) +0.80 2 H20(1) + 2 e — H2(8) + 2 OH+ (aq) AgBr(s) + - Ag(s) + Br" (aq) +0.10 HO2...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
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> This helps partially but the Ecell and pH is wrong.
mochi12 Mon, Dec 6, 2021 2:10 PM