A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º 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 1. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ Fº K - 16 A 1 90. kJ/mol 1.71 x 10 O 0.93 V B 1 108. kJ/mol 8.33 x 10 O - 1.12 V C 1 -69. kJ/mol 8.16 x 10 O 0.71 V O OO 18 -13 O O

The answer is (C), but why is (D) correct? Why would the negative ions in the salt bridge have to move from "the silver half-cell" to the copper half-cell? Don't the negative ions of whatever compound is in the whole of the salt bridge move to the copper half-cell? Maybe I'm just reading this too closely, let me know. Thanks!

Use this information to complete the table below.

A reaction has a standard free energy change of -15.0 kJ mol-¹. What is the equilibrium constant of the reaction at 25 °C?

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. me 1. ? • The cell potential under standard conditions E°. 00 2. His results are listed below. Ex 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. 000 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. 10 Ar cell n calculated quantities (Check the box next to any that are wrong.) K 0 E 27 A 2 156. kJ/mol O 2.14 X 10 0.81 V 11 B 2 66. kJ/mol O 3.65 × 10 -0.34 V C 2 -264. kJ/mol 46 1.78 x 10 -1.37 V K So Na G 4. 3.

A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG • 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 1. cell A B C₁ n 1 1. 1 calculated quantities (Check the box next to any that are wrong.) ·a AG 77. kJ/mol O 64. kJ/mol 35. kJ/mol O O K 3.09 X 10 6:13 X 10 13. 6 1.35 X 10 - 12. O X 0. 0.80 V 0.66 V -0.36 V Ś

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.

A student determines the value of the equilibrium constant to be 1.87x107 for the following reaction. Fe(s) + 2HCI(aq)- →FECI2(s) + H2(g) Based on this value of Keg: AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.39 moles of Fe(s) at standard conditions at 298K. kJ rxn