A voltaic cell is constructed with two Zn2+−ZnZn2+−Zn electrodes. The two cell compartments have [Zn2+]=[Zn2+]= 1.9 MM and [Zn2+]=[Zn2+]= 1.00×10−2 MM , respectively. What is the standard emf of the cell? What is the cell emf for the concentrations given?

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn" (aq)+Ba (s) → Sn (s)+ Ba* (aq) Suppose the cell is prepared with 2.11 M Sn 2+ in one half-cell and 3.16 M Ba 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. Ox10 미미

What is the cell potential for a voltaic cell having one electrode composed of a Cu strip dipped in a 0.11 M HCl(aq) solution and the other electrode composed of a Cu strip dipped in a 0.028 M HCl(aq) solution? Assume all other cell components are in place and the temperature is 25.0°C. Type your numeric answer and submit

Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left half-cell contains 0.115 M Cu(NO₃)₂ (aq). Express your answer to three significant figures.

Write the balanced chemical equation for the spontaneous redox reaction. Include states of matter. Calculate the standard cell potential.  If the initial concentrations of Zn2+ and of OH– are 1.0 × 10–7 and 2.0 × 10–7, respectively, calculate the cell potential after the Zn2+ concentration has increased by a factor of 100. At this point, what percentage of the initial voltage remains?

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)| H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for is –0.76 V. (Enter your answer to two significant figures.) pH =

I need to find standard cell potential, the non-standard cell potential, using [Au^+]= 0.0015M and [Fe^3+]= 0.033M.  I need to calculate Gibb's free energy and equilibrium constant, K.  Is the reaction spontaneous or nonspontaneous?  Are reactants or products favored at equilibrium under non-standard conditions?

A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X

The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V. If [Au³+] = 0.50 M, what is the concentration of Cu2+? (R = 8.314 J/K mol, F = 96,500 C.mol-¹) 3Cu + 2Au3+→ 3℃u²+ + 2Au O 1.61 M O1.37 M O 258 M O 5.16 M

A voltaic cell is being constructed from an Al/A|^ 3+ electrode and a Sn/Sn^ 2+ electrodeWhen constructed properly and the circuit is closed, the tin electrode is observed to gain mass and the overall cell potential to be 1.52V.  Which of the following chemical reactions takes place at the cathode? Al3+(aq) + 3e- → Al(s) Sn(s) → Sn2+(aq) + 2e-  Sn2+(aq) + 2e- → Sn(s) Al(s) → Al3+(aq) + 3e-  Based on the overall reaction taking place across the voltaic cell, how many moles of electrons are involved?  When electrons are flowing in the cell, which electrode gains mass? True or false:  If an aluminum electrode is set to be part of a voltaic cell that also involves a standard hydrogen electrode (SHE), the aluminum electrode would be the anode.