, calculate the standard reaction free energy AG° for the following redox reaction.

For the delta Go values given, determine the standard cell potential for the cell. 12 kJ/mol, n=3 and -45 kJ/mol, n=1.

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 following galvanic cells. Diagram I Au- 1.0 M Au³+ chemPad XX 80 1.16 80 (b) balanced cell equation II chemPad X V For each galvanic cell, give the balanced cell reaction and determine &. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) (a) balanced cell equation I 1.4 1.0 M Cu+ 1.0 M Cu²+ Au(s)+3Cu²+(aq) ⇒ Au³+(aq)+3Cu+(aq) |Au(s)+3Cu^2+(aq)Au^3+(aq)+3Cu^+(aq) Your answer indicates a reaction progressing in an inconsistent direction. -Pt Greek V i Diagram II Greek Cd- 1.0 M Cd2+ XX Enter a number. Cd(s)+2VO₂²+ (aq)+4H*(aq) ← Cd²+(aq)+2VO²+ (aq)+2H₂O(l) Cd(s)+2VO_2^2+(aq)+4H^+(aq)<--Cd^2+(aq)+2VO^2+(aq)+2H_2O(l) Your answer indicates a reaction progressing in an inconsistent direction. Help Help -Pt 1.0 M VO₂ 1.0 MH+ 1.0 M VO²+ i

Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)

When comparing the electrode potential values for the following equations, which reaction more likely undergoes oxidation and which more likely undergoes reduction? Based upon the electrode potentials which electrode is the anode and which is the cathode?

Summarize the process of predicting Spontaneous Direction for Redox Reactions?

5. Consider a redox reaction for which AG° is positive. Which of the following is true? (a) The reaction is spontaneous under standard conditions, K>1, and E° >0 (b) The reaction is spontaneous under standard conditions, K1, and E° >0 (d) The reaction is nonspontaneous under standard conditions, K<1, and E° <0

A certain metal M forms a soluble nitrate salt M(NO,) . Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of M(NO,), and the right half cell with a 15.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. O left Which electrode will be positive? O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

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