Consider the following cell notation and use a Table of Standard Electrode Potentials  to answer the question below Cd(s)|Cd2+(aq) || Cu2+(aq ) | Cu(s)  What would you change to increase the Ecell decrease Cd2+concentration decrease Cu2+concentration increase Cd2+concentration increase concentration of both ions decrease concentration of both ions

Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations. Co(s)|Co #(aq, 0.0155 M) || Ag*(aq, 1.50 M)|Ag(s) net cell equation:

If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2 is 1.00 atm, calculate the cell potential at 25.0°C.

› Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard reduction potentials. 2 Au³ +(aq) + 3 Ni(s) = 2 Au(s) + 3 Ni² + (aq) AGⓇ = kJ

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;…

Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s) From the table of standard reduction potentials: Cu²+/Cu 0.337 V, E₁₂/1 Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:I AGO for this reaction would be than zero. = = 0.535 V

What is the corresponding standard cell potential for the fllowing standard free energy change and electron stoichiometry value? 12 kJ/mol, n=3 A) -0.1242 V B) 0.0414 V c) -0.0414 V 96,485 V