Calculate Ecell for the following reaction and conditions: 0.50 M Br2 (aq), 0.10 M Pb+2 (aq), 0.30 M Br- (aq).
Br2(aq) + Pb(s) --> Br- (aq) + Pb+2 (aq)……(unbalanced).
Calculate Ecell for the following reaction and conditions: 0.50 M Br2 (aq), 0.10 M Pb+2 (aq),...
Calculate the cell potential (Ecell) and Gibbs Free Energy (Delta G) for the reaction (2Ag+ (aq) + Fe (s) -> Fe2+ (aq) + 2Ag (s) ) under these conditions: a 250mL beaker of 1.0mol Fe metal electrode and 0.10 moles of Fe 2+; and a second 250mL beaker of 2.0 moles Ag metal electrode ad 0.50 moles of Ag+. E naught of the cell= 1.21 V.
Calculate the value of Ecell at 25 °C for the following reaction and conditions: 2 Al(s) + 3 12(s) — 2 A13+(aq) + 6 1'(aq) E cell = 2.20 V and [A13+) = 4.5 x 10-3 M and [I"] 0.15 M. A. 2.10 V B.2.39 V OC. 2.30 V OD.2.20 V E. 2.23 V
The following electrochemical cell was set up in the lab Ag(s)│Ag(NO3)(aq)││KMnO4(aq), HCl(aq), Mn(Cl)2(aq)│Pt(s) What is Ecell° for this galvanic cell? If a more complete description of the cell is Ag(s)│Ag(NO3)(aq, 0.50 M)││KMnO4(aq, 0.50 M), HCl(aq, 2.5 M), Mn(Cl)2(aq, 0.01 M)│Pt(s), Ag(s) what is Ecell? What is the balanced, spontaneous cell reaction for the cell conditions given in b.?
Calculate Ecell for Pb(s) | PbSO4(s) | Pb2+(aq) || Cu2+(aq) | Cu(s) the way it is written here given Cu2+(aq) + 2 e- → Cu(s) E° = +0.337 V PbSO4(s) + 2 e- → Pb(s) + SO42-(aq) E° = -0.356 V
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of 0.10 M with a platinum electrode and the second compartment has Cr3+ at a concentration of 0.20 M and a Cr electrode. Use the following reduction potentials to answer the questions: Cr3+ (aq) + e ̄→Cr(s) εo = - 0.73 V Br2(aq) + 2e ̄→2Br ̄ (aq) εo =1.09V a. What is the standard cell potential for...
(C) 5, product 16. Which reaction has Standard Reduction Potentials, y Pb2+(aq) + 2e--+ Pb(s) -0.13 Sn (aq) +2e Sn2 (aq) +0.15 Br (aq) + 2e- 2Br(aq) +1.09 the highest potential under standard conditions? (A) Sn (aq)+ Pb(s)- products (B) Br (aq) +Sn (aq) products (C) Pb(s)+ Br2(aq) products (D) Pb?'(aq)+ Sn (aq) products homical cell is set un as shown.
2. Balance the following reaction under acidic conditions. Cl2(aq) + Br2(1) BrO3-(aq) + Cl-(aq)
QUESTION 27 Calculate Ecell under non-standard conditions for the following electrochemical cell: Pt(s)| FeCl2 (aq, 0.150 M), FeCl3 (aq, 0.050 M) || Cl2 (9, 1 atm), NaCl (aq, 0.075 M) | Pt (s) -1.60 V 0.72 v 0.69 V -1.79 V 0.62 V none of these
Sketch a diagram of a galvanic cell represented by the following shorthand notation: Pb(s)|Pb2+ (aq)||Br2(1), Br (aq)|Pt(s) Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. e e → Group 1 2Br - Group 3 (anode) Pb2+ Salt bridge NaNO, Group 3 (cathode) Br2 NO3- Group 2 Na+ Group 2 Group 2 Pb Group 2 Group 2 Pt
Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures. Consider the following reaction. Mg(s)+2Vo; (aq)+ 4 H* (aq)Mg2+(ag)+ 2 VO2 (aq)+ H2O(l) Ecell 3.37 V. Part A Calculate the AGo for the reaction. Express your answer to three significant figures.