What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL?
What would happen to the measured cell potentials if 30 mL solution was used in each...
What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL? will rate, thanks!
EXPERIMENT 1: List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you expect given electrochemical cell to be spontaneous or nonspontaneous? Explain your answer. Pb|Pb(NO3)2||Zn|Zn(NO3)2 EXPERIMENT 1: What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL? EXPERIMENT 1: Calculate the theoretical standard cell potential for the electrochemical cell that includes the reaction. Mn+Pb2+⟶Mn2++Pb The standard reduction potentials for each half reaction are...
Do measured cell potentials show any effect of solution concentration on cell potential for the reactions performed in this experiment? For example, would the potential have changed for 0.1 M solutions from standard conditions of 1 M solutions. Yes, the Nernst equation shows potential is dependent on solution concentrations. No, the Nernst equation does not show potential is dependent on solution concentrations. The potential would change if the cathode and anode were mislabeled. Potential is dependent on concentration, but in...
6. What would be the effect on measured cell potential if some solution in one well spilled over and mixed with that in the other well? For example, suppose some Cu solution spilled into the compartment with the zinc elecrode and Zn solution. (Consider possible interactions that might now happen.)
4(d) Explain briefly how standard half-cell reduction potentials are actually measured.
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
EXPERIMENT 1: What do you think will happen to the temperature if you used 75 mL of HCl and 75 mL of NaOH instead of the 10 mL each you used in Experiment 1?
POST-LAB QUESTIONS 1. What would happen if you added more than 5 mL of yeast solution to the H2O2? 2. What would happen if you added more than 5 mL of H2O2 to the 5 mL of yeast solution?
A 25 ml solution of Quinine has an absorbance of 0.525 when measured in a 2.00cm cell. When 3 millimoles are added to the solution the absorbance increases to 0.875. What is the number of moles in the original solution.