When the Hg2+ concentration is 2.39×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.509V. What is the Zn2+ concentration? Hg2+(aq) + Zn(s) Hg(l) + Zn2+(aq) Answer:       M

When the Hg2+ concentration is 2.22×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.486V. What is the Cr³+ concentration? 3Hg²*(aq) + 2Cr(s)3Hg(1) + 2C1³*(aq) Answer: M

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 H₂ pressure is 9.18x10-3 atm, the H+ concentration is 1.35M, and the Pb2+ concentration is 3.44x10-4M ? 2H+ (aq) + Pb(s)→ H₂(g) + Pb²+ (aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Submit Answer V O Search Retry Entire Group 9 more group attempts remaining I Previous Next Save an

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

When the Pb2+ concentration is 1.15 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.609V. What is the AI3+ concentration? 3PB2+(aq) + 2AI(s)3Pb(s) + 2AI3+(aq) Answer: M