11. Determine the cell notation for the redox reaction given below. 3 Cl2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe3+(aq) A) Cl2(g) ∣ Cl⁻(aq) ∣ Pt ll Fe(s) ∣ Fe3+(aq) B) Cl⁻(aq) ∣ Cl2(g) ∣ Pt ll Fe3+(aq) ∣ Fe(s) C) Fe3+(aq) ∣ Fe(s) ll Cl⁻(aq) ∣ Cl2(g) ∣ Pt D) Fe(s) ∣ Cl2(g) ll Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt E) Fe(s) ∣ Fe3+(aq) ll Cl2(g) ∣ Cl⁻(aq) ∣ P

What is the oxidizing agent in the redox reaction represented by the following cell notation?             Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt

Using standard reduction potentials from the ALEKS Deta tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. Cu (aq) + HNO₂ (aq) + H* (aq) → Cu² (aq) + NO(g) + H₂O (1) X

Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…