When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.279V. What is the Mg?+ concentration? 2Ag*(aq) + Mg(s)- →2Ag(s) + Mg²*(aq) Answer: M

us the tabulated half cell potentials to calculate ▲G° for the following redox reaction 2Al(s) + 3Mg2+(aq) --> 2Al3+(aq) +3Mg(s)

When the Pb²+ concentration is 5.44×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.953V. What is the Mn²+ concentration? Pb²+ (aq) + Mn(s) Pb(s) + Mn²¹(aq) Answer: M

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.46 atm, the F" concentration is 6.08×10-3M, and the Pb2+ concentration is 5.78×10-4M ? F2(g) + Pb(s)- →2F*(aq) + Pb²+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

When the Hg2+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 3.335V. What is the Mg2+ concentration?Hg2+(aq) + Mg(s) =>Hg(l) + Mg2+(aq)Answer:  M

Salt bridge A concentration cell similar to the one shown is composed of two Cr electrodes and solutions of different Cr3+ concentrations. The left compartment contains 0.222 M Cr3+ , and the right compartment contains 0.729 M Cr3+ . Calculate the cell potential for this reaction at 298 K. volts In this chromium concentration cell, the reaction would proceed spontaneously

What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 8.22×10-4 atm, the F concentration is 1.46M, and the Cr³+ concentration is 1.01M? 3F₂(g) + 2Cr(s)—6F¯(aq) + 2Cr³+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: