General Chemistry
Improve your experience by picking them
Consider the galvanic cell shown below with a potential of 1.369 V at 25°C
Pb(s) | PbCl2(s) | Cl–(0.20 M) || Cr2O72–(0.20 M), Cr3+(0.20 M), H+(0.20 M) | Pt(s)
Determine the Ksp value for PbCl2(s).
Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(l) E°red = 1.232 VPb2+(aq) + 2 e– → Pb(s) E°red = –0.126 V
Consider the following cell:
Co(s) | Co2+ (2.0 M) || H+(? M) | H2( 1.0 atm) | Pt(s)
Calculate the pH of the solution in the cathode compartment if the observed potential of the cell is 0.14 V at 25 °C. (E°Co2+ = − 0.28 V)
Pt (s) | H2(g, 0.839 atm) | H+ (aq, ? M) || Cr2+ (aq, 1.50 M) | Cr(s)
Calculate the H+ concentration at 25 °C given that the Ecell = -0.847 V
Use the following reduction potential values:
2 H+(aq) + 2e- → H2(g) E° = 0.00 V
Cr2+ (aq) + 2e- → Cr(s) E° = -0.913 V
An electrochemical is depicted with the cell notation Cu | Cu2+ || Mn3+ | Mn2+ | Pt. Draw the cell and show the flow of electrons and ions.
For the given cell notation, write an overall cell reaction:
Mn(s) | Mn2+(aq) || Fe2+(aq) | Fe(s)
Draw the cell diagram, label which electrode is the anode and the cathode. Draw arrows to show the directions in which the ions and electrons flow.
A galvanic cell is made up of a Zn/Zn2+ anode and Pb/Pb2+ cathode connected together by a wire. A salt bridge also connects the two cells. Write a cell notation for this galvanic cell.
Consider the following redox reaction:
2 NH4+(aq) + MnO4−(aq) → 2 MnO2(s) + N2(g) + 4 H2O(l)
Write a shorthand notation for this reaction. In your notation, you can use an inert metal if necessary.
Ni(s) | Ni2+(aq) || Br2(l) | Br−(aq) | Pt(s)
Explain why we need an inert electrode at the cathode.
Write a shorthand notation for the following electrochemical cell:
Consider the following cell notation:
Mg(s) | Mg2+(aq) || Cu2+(aq) | Cu(s)
Determine the Mg2+:Cu2+ concentration ratio at 25.0 °C if the cell potential is measured to be 2.74 V. (E°red,Mg2+ = −2.37 V; E°red,Cu2+ = 0.34 V)
The galvanic cell, Mg(s) | Mg2+(aq) || Ce4+(aq), Ce3+(aq)| Pt(s), has a standard potential of 0.870 V. Provide the standard reduction potential for the Ce4+/Ce3+ half-cell.
For the given electrochemical cell, cell potential is dependent on the copper concentration in the cathode half-cell.Pt(s) | H2(g, 1.0 atm) | H+(aq, 1.0 M) || Cu+(aq, ? M) | Cu(s)This cell has an Ecell of 0.34 V. Determine the [Cu+] of the solution.
Calculate the E°cell of the following celll:
Fe(s) | Fe3+(aq) || Cl2(g) | Cl-(aq) | Pt(s)
Write the cell notation for the reaction below:
3 Cu2+(aq) + 2 Al(s) ↔ 3 Cu(s) + 2 Al3+(aq)
Identify and balance the reaction for the following cell:
Pb(s) | Pb2+(aq) || NO(g) | NO3-(aq),H+(aq) | Pt(s)
For the given electrochemical cell, cell potential is dependent on the pH of the solution.
Pt(s) | H2(g, 1.0 atm) | H+(aq, ? M) || Ag+(aq, 1.0 M) | Ag(s)
This cell has an Ecell of 923 mV. Determine the pH of the solution.
The cell potential of this electrochemical cell depends on the pH of the solution in the anode half-cell.
Pt(s) | H2(g, 1 atm) | H+(aq, ? M) || Cu2+(aq, 1.0 M) | Cu(s)
What is the pH of the solution if Ecell is 355 mV?