A current of 5.0 A was passed through an electrolytic cell containing molten BaCl2 for 90 min. The following redox reaction took place. 2 Cl– + Ba2+  →  Cl2  +  Ba MM of Ba = 137.3 g/mol MM of Cl2 = 70.9 g/mol R = 8.314 J/mol∙K F = 96,485 J/mol∙V How many moles of electrons passed through the cell? a. 7.77 x 10-5 b. 16.8 x 101 c. 4.66 x 10-3 d. 2.80 x 10-1 e. 5.36 x 103

(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification 2+ Hg (aq) + 2e- →Hg(1) Sn(s) Sn²*(aq) + 2e (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients.

6. As we will discuss when we get to the chapter on electrochemistry, the AGO for a reaction can very easily be determined by incorporating the reaction into an electrochemical cell (battery). AGO is directly proportional to the potential (voltage) of the cell. Using this technique, it was found that the AG° = -1370.8 kJ for the following reaction. 2 CH₂OH(1) + 3 0₂(g) → 2 CO₂(g) + 4H₂O(1) 0. The standard entropy change (AST) for this reaction is ?163.6 J/K at 25.0 °C. A. B. C. What is the standard enthalpy of reaction, AHxn at 25.0 °C?. Please provider your answer below. ☐☐ → 0 0 0 If AHrxn and ASrxn do NOT change with temperature, what is the AGxn at 171.58 °C? Please provider your answer below. 0² 0₂ 010 H 0² 0₂ Above Please provider your answer below. °C, the reaction will become non-spontaneous? kJ kJ

Calculate the standard Gibbs free energy change value (AG°rxn) in kJ/mol associated with the following unbalanced redox process: (3 sf) Ni²+ (aq) + Cr (s) → Ni (s) + Cr3+ (aq) Type your answer...

Balance the redox reaction by inserting the appropriate coefficients. redox reaction: 4H+ClO2−+2I−⟶Cl−+2H2O+I2−

1:17 Question 11 of 17 Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard Reduction Potentials Cu²+ (aq) + e → Cu*(aq) V2+ (aq) + 2e → V(s) Mg²+ (aq) + 2e → Mg(s) E° (V) 0.15 -1.18 -2.37 A) V²+ + 2Cu* → V + 2Cu²+ B) Mg2+ + V→ V²+ + Mg C) Mg²+ + 2Cu* → 2Cu²+ + Mg D) Mg2+ + V²+→ Mg + V E) V + 2Cu²+ → V²+ + 2Cu* Submit Periodic Table

› Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Ni²+] = 0.00100 M and [Au³+] = 0.834 M. Standard reduction potentials can be found in this table. 3 Ni(s) + 2 Au³ +(aq) — 3 Ni² †(aq) + 2 Au(s) E = 1.72 Incorrect V

The standard EMF for the cell using the overall cell reaction below is +0.65 V: 2AI (s) + 312 (s) What is AGO for the cell reaction in kJ? Express your answer in decimal notation to one decimal place, without units. 2A1³+ (aq) + 61¯ (aq) →>>

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --

What are the oxidation and reduction half reactions in the following redox reaction: 2Al(s) + 3Pt(NO3)2(aq) → 3Pt(s) + 2AL(NO3)3(aq) Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE V Al(s) → Al3+(aq) + 3e a b Pt2+ (aq) + 2e-→ Pt(s) Al3+(aq) + 3e' → Al(s) d Pt(s) → Pt2+(aq) + 2e-