Which of the following is/are TRUE about Galvanic cell? I. The Gibbs Free Energy of the cell is negative. II. It requires an external source of energy such as.a 9-V battery. III. The energy transformation is from chemical to electrical energy. IV. The electromotive force of the cell is greater than zero. II, IV I, II, II I, II, IV I, II, IV

You are a bioengineer designing a new type of pacemaker. Which type of Galvanic cell would be best for you to use in this new device?

The standard cell potential (E°cell) of the reaction below is -0.55 V. The value of A G° for the reaction is J/mol. 12 (s) + 2Br" (aq) → 21 (aq) + Br2 (1) 0.55 5.5 · 5. 10-6 1.1· 105 0.54 none of the above

A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGO. . • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. cell n A B U 2 2 2 calculated quantities (Check the box next to any that are wrong.) AGⓇ 64, kJ/mol O -160, kJ/mol -228. kJ/mol O O K -12 6.13 X 10 O -29 9.32 × 10 O 1.14 X 10 40 O 0 E 0.33 V 0.83 V 1.18 V O O G o

Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=

Consider the following galvanic cell:     E° (V) U3+  +  3 e−   →   U(s) −1.642 In3+  +  2e−   →   In+ −0.444 The electron flow is clockwise electrons don't move in this galvanic cell counterclockwise

Consider the cell below. Please note that this cell may or may not obey the conventions of a standard cell diagram. Assume the cell is working spontancously under standard conditions. A B Salt bridge H. K. Image: Rectangle I in a beaker in a solution of J. An arrow F points away from rectangle I and an arrow E points toward rectangle I. The rectangle I is joined by a line another rectangle L in a separate beaker. On this line, an arrow labelled A points toward I and an arrow labelled B points to L. Rectangle L in a beaker in a solution of K. An arrow H points away from rectangle Land an arrow G points toward rectangle L.A salt bridge joins the beakers. On this salt bridge, an arrow labelled C points toward I and an arrow labelled D points to L. End of image. | = Q J = QNO3 Reduction Potential Q = minus 0.400 V K = RNO3 Reduction Potential R = minus 0.200 V L = R Match the each statement to the letter that best describes it. Some answers may be used more than once. of: C. E.

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

Which statement about electrolytic cells is false? Electrolytic cells convert electrical energy into chemical energy. O The redox reaction is non-spontaneous. The anode and cathode are placed in the same container with the aqueous electrolyte. O The anode is negative and the cathode is positive. O The external battery supplies the electrons.