1. Calculate the value of E° for the reaction below; Pb2+ (aq) + Ni (s) → Ni2+(aq) + Pb (s)
2. Calculate the value of ΔG° for the reaction below using your value from Question one; Pb2+ (aq) + Ni (s) → Ni2+(aq) + Pb (s)
3. Balance the following redox reaction in acidic conditions; KMnO4 (aq) + NO (g) → MnO2 (s) + NO2(g)
1. Calculate the value of E° for the reaction below; Pb2+ (aq) + Ni (s) →...
1. Balance the following redox reaction in acidic conditions; KMnO4 (aq) + NO (g) → MnO2 (s) + NO2(g) (Please show every step when balancing this redox reaction in acidic condition, thanks.) 2. Which chemical has more entropy and explain why. Linear polyethylene (s) or hyperbranched polyethylene (s)
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Consider the following reaction at 298K. Pb2+ (aq) + Ni (s) → Pb (s) + Ni2+ (aq) Which of the following statements are correct? Choose all that apply. OK 1 delta Gº > 0 n= 5 mol electrons The reaction is product-favored. Eºcell > 0 Submit Answer Retry Entire Group 9 more group attempts remaining
1. which of the following is the strongest oxidizing agent? (in an acidic solution) (pick one) PbO2(s) Mg(s) Ba2+(aq) NO3-(aq) MnO2(s) 2. what element is being oxidized in the following redox reaction? Co2+(aq)+NH4+(aq)=Co(s)+NO3-(aq) Choices are: O,N,Co,Xe, or H 3. which of the following reactant pairs would result in a spontaneous redox reaction? (pick one) Al(s)+Pb2+(aq) Pb(s)+Mn2+(aq) Ni(s)+Zn2+(aq) Ag(s)+Ni2+(aq)
Using the following standard reduction potentials Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions. Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s) Group of answer choices E° = -0.90 V, spontaneous E° = -0.90 V, nonspontaneous E° = +0.90 V, nonspontaneous E° = +0.90...
Balance each redox reaction occurring in acidic aqueous solution. a. PbO2(s) + (aq) Pb2+(aq) + 12(s) b. SO32-(aq) + MnO4 (aq) — 3042-(aq) + Mn²+(aq) c. S2032-(aq) + Cl2(g) 8042-(aq) + Cl²(aq)
electro Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq)
question. Consider the following reaction at 298K. Pb2+ (aq) + Co (s) Pb (s) + Co2+ (aq) Which of the following statements are correct? Choose all that apply. OK<1 On= 5 mol electrons E cell <0 The reaction is product-favored. delta Gº<0 Submit Answer Retry Entire Group 4 more group attempts remaining Consider the following reaction at 298K. Ni2+ (aq) + Pb (8) -Ni (6) + Pb2+ (aq) Which of the following statements are correct? Choose all that apply. AG°...
Two standard reduction potentials are given below. Pb2+(aq) + 2 e− → Pb(s) E⁰red = −0.126 V Cl2(g) + 2 e− → 2 Cl−(aq) E⁰red = +1.358 V (a) Which is a stronger reducing agent, Pb(s) or Cl−(aq)? Pb(s) ; or Cl−(aq) (b) Which is the most difficult to oxidize, Pb(s) or Cl−(aq)? Pb(s); or Cl−(aq) (c) Is Pb(s) able to reduce Cl2(g) in a spontaneous reaction? is able; or is not able (d) Is Cl−(aq) able to reduce Pb2+(aq)...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) 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...