The particle diagrams above represent NaCl(1) and its decomposition into Na(l) and Cl2(g) in an electrochemical cell after voltage is applied. Which of the following statements about the thermodynamic favorability of the decomposition of NaCl(1) is supported by the particle diagrams and why? The decomposition is thermodynamically favored because the transfer of electrons to and from the ions occurs at the electrodes. The decomposition is thermodynamically favored because the formation of a gaseous product results in an increase in entropy. The decomposition is not thermodynamically favored because the pure elements form only after electrical energy is supplied. D The decomposition is not thermodynamically favored because there is a decrease in the number of particles as the reaction proceeds.

The particle diagrams above represent NaCl(1) and its decomposition into Na(l) and Cl2(g) in an electrochemical cell after voltage is applied. Which of the following statements about the thermodynamic favorability of the decomposition of NaCl(1) is supported by the particle diagrams and why? The decomposition is thermodynamically favored because the transfer of electrons to and from the ions occurs at the electrodes. The decomposition is thermodynamically favored because the formation of a gaseous product results in an increase in entropy. The decomposition is not thermodynamically favored because the pure elements form only after electrical energy is supplied. D The decomposition is not thermodynamically favored because there is a decrease in the number of particles as the reaction proceeds.

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...

See similar textbooks

Similar questions

Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation: M| M+||N3+|N with reduction potential of 0.36 V for M and 1.05 V for N, respectively. (Note that M and N are fake metals). Calculate the value of ∆G° in J. F = 96500 C/mol e- Enter your answer in scientific notation with 2 decimal places and be sure to include the correct sign. Example: -2.34e+6 or 1.23e-5. Note e is used for "x10" in this notation! Do NOT type "x 10"!
Predict the products of the following single replacement reaction and predict whether it will be spontaneous. Fe(s) + 2AgNO3(aq) →
Give a clear explanation handwritten answer ...
Molten RbCl can be electrolyzed to form metallic Rb. For what duration should an electrolysis be performed at a current of 1.98 A in order to produce 13.4 g Rb?
Determine the standard free energy change, ΔG°f , for the formation of S2−(aq) given that the ΔG°f for Ag+(aq) and Ag2S(s) are 77.1 kJ/mole and −39.5 kJ/mole respectively, and the solubility product for Ag2S(s) is 8 × 10−51.
Consider the following reaction at 298K.2 Cu2+ (aq) + Co (s) 2 Cu+ (aq) + Co2+ (aq)Which of the following statements are correct?Choose all that apply. K < 1 n = 4 mol electrons The reaction is product-favored. Eocell > 0 delta Go > 0
Calculate the G in kJ for the following cell: Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Eocell=+1.59 V Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Group of answer choices -473 -374 -158 -734 -658 Calculate Ecell in volts. Cu(s)|Cu2+(3.00x10-4)||Ag+(0.15M)|Zn(s) Eocell=+0.620 V 0.700 0.544 0.944 0.644 0.800
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the cell potential (Ecell), in volts, for this reaction at 35.4 °C when [M+] = 0.00533 M and [N2+] = 0.725 M? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) E°cell = 0.128 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 2. calculated quantities (Check the box next to any that are wrong.) cell n AG K E - 16 1.14 X 10 A 2 -91. kJ/mol -0.47 V - 49 1.98 x 10 B 2 - 278. kJ/mol 1.44 V - 44 5.34 x 10 2 247. kJ/mol 1.28 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
What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0235 V and n = 2?(F = 96,500 J/(V･mol), R = 8.314 J/(mol･K))
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. any. 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 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 n A B C 1 calculated quantities (Check the box next to any that are wrong.) AGⓇ 37. kJ/mol - 66. kJ/mol -47. kJ/mol K 6 3.03 × 10 2.74 × 10 5.83 × 10 12 9 X 0 E -0.38 V 0.68 V -0.49 V S