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Calculate E°(cell) for the reaction, 2 103"(aq) + 10 Fe2+(aq) <=> 10 Fe3* (aq) + typen...
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+ (aq) + 2 C1 (aq) Write a cell diagram for this reaction In this reaction, calculate Eºcell under standard conditions Calculate AGº from the cell potential B. C. D. Calculate K from the cell potential. E. Predict the value of Ecell for this reaction in if the concentration of is 0.150 M, is 0.100 M and the concentration of Cl- is 0.010 M. Fe2+...
Half-reaction Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e - Fe(s) Fe3+ (aq) - Fe2+ (5) Sn+ (aq) + 2e - Sn2(aq) E (V) -0.74 -0.440 +0.771 +0.154 1. Calculate the standard cell potential for the voltaic cell based on the reaction below, given the table above: 35nt(s) + 2Cr (s) - 2 C (s) + 3 Sn () ANSWER: 2. Calculate the standard cell potential for the voltaic cell based on the reaction below, Riven the table above 3Feb...
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...
Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential is 0.683 V, what is the ratio of Fe2+(aq) to Fe3+(aq)? What is the ratio of these concentrations if the cell potential is 0.807 V?
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr(s) -0.74 Fe2+ (aq) + 2e- Fe (5) -0.440 Fe3+ (aq) + e - Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. 35n4+ (aq) + 2Cr (s) → 2Cr3+ (aq) + 3Sn2+ (aq) A) +1.94 B) +0.89 C) +2.53 D) -0.59 E) -1.02
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
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?
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
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)
Given the cell reaction: 2Cl–(aq) + Fe3+(aq) → Cl2(aq) + Fe2+(aq): (unbalanced) a) As written, is the cell galvanic or electrolytic? b) Calculate ε°cell. c) Calculate ΔG°.