Calculate the voltage of the cell you would expect to measure using your Hg st

Consider the cell described below. Al | Al³+ (1.00 M) || Pb²+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al³+] to have changed by 0.45 mol/L. (Assume T= 25°C.) V Need Help? Read It Watch It

Using the standard reduction potentials here, calculate the standard potential for the following cell in V (make sure you don't round your answer): Culs)Cu2"(aq)||Mn2 (aq).H"(aq)|MnO2(s)Pt(s) Your Answer:

A Zn/Zn^2+ concentration cell has a voltage of 0.078 V at 25 deg C. The concentration of Zn ^2 + in the cathode is 5.2 x 10^-3 mol L-1 What is the concentration of Zn ^2+ in the anode?

A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown.  a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s).  b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+

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