A student made measurements on some electrochemical cells and calculated three quantities:• The standard reaction free energyAGº.• The equilibrium constant K at 25.0 °C.• The cell potential under standard conditions E".His results are listed below.oloUnfortunately, 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.ArNote: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, youcorrect.ay assume the number of significant digits in each quantity isAlso note: for each cell, the number n of electrons transferred per redox reaction is 2.calculated quantities(Check the box next to any that are wrong.)cellKE30A2174. kJ/mol3.04 X 10-0.90 V39В2- 224. kJ/mol1.75 X 10- 1.16 V- 338.71 X 10C2183. kJ/mol-0.95 V

Here we have to predict the incorrect value of any quantities from the given data.

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". 圖 His results are listed below. ol. 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. calculated quantities (Check the box next to any that are wrong.) cell n aG E K 174. kJ/mol 30 3.04 X 10 A -0.90 V 39 1.75 x 10 B 2 - 224. kJ/mol -1.16 V -33 8.71 x 10 2 - 183. kJ/mol -0.95 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". 圖 His results are listed below. ol. 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. calculated quantities (Check the box next to any that are wrong.) cell n aG E K 174. kJ/mol 30 3.04 X 10 A -0.90 V 39 1.75 x 10 B 2 - 224. kJ/mol -1.16 V -33 8.71 x 10 2 - 183. kJ/mol -0.95 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student made measurements on some electrochemical cells and calculated three quantities: AG. • The equilibrium constant K at 25.0 °C. • The standard reaction free energy • The cell potential under standard conditions 圖 His results are listed below. dlo 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 AG K E 8- A -41. kJ/mol 6.56 x 10 -0.42 V 15 8.76 x 10 1 -91. kJ/mol - 0.94 V 17 1.52 x 10 1 -96. kJ/mol - 1.00 V Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility MAY 8. MacBoo B.
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". 圖 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. do 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. calculated quantities (Check the box next to any that are wrong.) cell AG° E K A 2 268. kJ/mol O 46 8.95 x 10 -1.39 V -38 B -212. kJ/mol 7.23 x 10 1.10 V 27 2.14 x 10 2 -156. kJ/mol O -0.81 V Explanation Check Privacy Accessibility 02021 McGraw-Hill Education. All Rights Reserved. Terms of Use MacBook Air F12 ►► FI F10 F9 F7…
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. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ ΔG K Eº - 32 A 2 А -178. kJ/mol 6.54 × 10 -0.92 V B 179. kJ/mol 2.29 X 10 -0.93 V с 2 127. kJ/mol 1.78 × 10²2 0.66 V 31 X ?
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 2. calculated quantities (Check the box next to any that are wrong.) cell AG K E A 181. kJ/mol 5.13 x 10 -0.94 V 162. kJ/mol 2.41 x 10 0.84 V 66. kJ/mol 3.65 x 10 0.34 V Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Ac MAY 8. 2. 2. 2.
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) | Sn² + (0.0062 M). Sn +(0.15 M) || Fe +(0.11 M), Fe²+(0.0045 M) | Pt(s) ES' *Sn²+ = 0.154 V EF = 0.771 V Ecell 0.613 Incorrect Is the electrochemical cell spontaneous or not spontaneous as written at 25 "C? spontaneous not spontaneous
If allowed to run undisturbed, how will the potential of a concentration cell change over time? It will increase. It will stay the same. It will decrease.
I. For each of the following; a. Write the overall cell reaction/ cell representation b. Calculate the standard cell potential (Eo) c. Determine whether the reaction is spontaneous or non-spontaneous. Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) Pb(s) + Sn+2(aq) → Pb+2(aq) + Sn(s) Al / Al+3 // Mg+2 / Mg Ca / Ca+2 // Cr+3 / Cr
The Nernst equation can be used to calculate... A. cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard B. standard cell potentials from standard reduction potentials C. cell potentials given only the temperature and reactant concentrations D. cell potentials from standard oxidation potentials E. the change in standard Gibbs free energy from standard cell potentials
Please don't provide handwritten solution .....
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 AGº K A 1 -19. kJ/mol 4.69 × 10 0 E 0.20 V 13 B 1 77. kJ/mol 3.09 × 10 0.80 V -14 C 1 75. kJ/mol 7.25 X 10 0.78 V
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) :+1.065 V (red Cro, (aq)+4 H,O(1)+3e Cr(OH)3(s)+5 OH (aq) -0.13 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode.
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 2. cell n A B C 2 2. 2 calculated quantities. (Check the box next to any that are wrong.) .0 AG 172. kJ/mol J 127. kJ/mol - 170. kJ/mol K -31 7.36 X 10 5:63 X.10 - 23 29 6.06 × 10 - O O E -0.89 V. 0:66 V -0.88. V 5