Use the following standard cell potentials to answer the questions below.
Fe3+(aq) + e− ⇌ Fe2+(aq) E° = 0.771 V
Ag3+(aq) + e− ⇌ Ag2+(aq) E° = 1.800 V
1. What is ΔG° (in kJ/mol) for this reaction? Report answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol)
2. This reaction is (spontaneous/not spontaneous)
Use the following standard cell potentials to answer the questions below. Fe3+(aq) + e− ⇌ Fe2+(aq)...
Use the reduction potentials and the unbalanced chemical equation below to answer the following questions: Mn2+ (aq) + Ag+ (aq) → Mn (s) + Ag2+ (aq) Half-cell reaction / E° (V) Mn2+(aq) + 2e− ⇌ Mn(s) / -1.185 Ag2+(aq) + e− ⇌ Ag+(aq) / 1.980 a) Determine E°cell (in V). Report your answer to three decimal places in standard notation (i.e. 1.234 V) b) Determine ΔG° (in kJ/mol). Report your answer to three significant figures in scientific notation (i.e. 1.23e4...
Ag3+(aq) + e− ⇌ Ag2+(aq)E° = 1.800 V2H+(aq) + 2e− ⇌ H2(g)E° = 0.000 V1. Answer the following questions under standard conditions(a) The half-cell containing Ag2+/Ag3+ is the cathode .(b) The half-cell containing H+/H2 is the anode .(c) What is E°cell (in V)? Report your answer to three decimal places in standard notation (i.e., 0.123 V).1.800 V(b) What is ΔG° (in kJ/mol) for the process that is occurring in the electrochemical cell? Report your answer to three significant figures in...
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...
Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77 V Pb2+ (aq) + 2 e. → Pb(s) E。--0.13 V Calculate the standard cell potential for the galvanie cell reaction given below, and determine whether or not this reaction is spostaneous under standard conditions. Pb2+ (aq) + 2 Fe2+ (aq) → 2 Fe3+ (aq) + Pb(s) ⓔ A. E.-0.90 V, nonspontaneous OB. E-0.90 V, spontaneous C. Eo +0.90 V, nonspontaneous OD0.90 V, spontaneous
Use the reduction potentials, the unbalanced half reactions and the unbalanced chemical equation below to answer the following questions: Reaction E° (V) In+(aq) + e− → In(s) -0.140 In3+(aq) + e− → In(s) -0.338 In(s) + In3+(aq) → In+(aq) + In(s) 1. Determine Ecell (in V) for this reaction in the direction shown. Report your answer to three decimal places in standard notation (i.e. 1.234 V). Tries 0/5 2. Determine ΔG° (in kJ) for this reaction. Report your answer to...
A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). emf of this cell under standard conditions E∘ = 0.771 V What is the emf for this cell when [Fe3+]= 3.70 M , PH2= 0.95 atm , [Fe2+]= 1.0×10−3 M , and the pH in both compartments is 3.95? Express your answer using two significant figures.
Answer the following questions related to the given electrochemical cell under standard conditions.W3+(aq) + 3e− ⇌ W(s)E° = 0.100 VCo2+(aq) + 2e− ⇌ Co(s)E° = -0.280 V1. Answer the following questions.(a) The half cell containing W/W3+ is the anode/ cathode(b) Which one of the following statements isTRUE for the half cell containing W and W3+.W3+ will be oxidized to form W.W3+ will be reduced to form W.W will be reduced to form W3+.W will be oxidized to form W3+.(c) The half...
Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V
The following standard reduction potentials have been determined for the aqueous chemistry of iron: Fe3 (a)e>Fe2-(aq 0.770 V Fe2 (aq) 2e>Fe(s E°-0.409 v Calculate the equilibrium constant (K) for the disproportionation of Fe2(aq) at 25 °C. Submit Answer 5 question attempts remaining
Part C Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction Zn(s) +Fe2(a)Zn2+ Fe(s) Report the answer in volts with three significant figures. LA Value Units Request Answer Submit Part D Determine the equilibrium constant for the above reaction Report to 1 significant figure and using scientific notation. ΑΣ Submit Request Answer