Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.5M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.19 volts. Your Answer:

Consider the following galvanic cell at 25°C. Pt | Cr²+ (0.25 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr²+ "(aq) + Co2+ Calculate the cell potential & for this galvanic cell and AG for the cell reaction at these conditions. + (aq) → 2 Cr³+ (aq) + Co(s) K = 2.79x107

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calculated quantities (Check the box next to any that are wrong.) 0 K 0 E cell n AG 44 A 2 -255. kJ/mol 4.72 x 10 О -1.32 V -31 B 2 - 176. kJ/mol 1.47 x 10 ○ -0.91 V 44 C 2 255. kJ/mol 4.72 x 10 -1.32 V ☑

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. calculated quantities (Check the box next to any that are wrong.) cell n 46° K 1 - 124. kJ/mol 5.30 x 10 21 -1.28 V -18 4.53 x 10 B 1 - 99. kJ/mol -1.03 V -7 2.20 x 10 1 - 38. kJ/mol 0.39 V

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

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 1. calculated quantities (Check the box next to any that are wrong.) cell n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V