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 madesome 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 celI, the number n of electrons transferred per redox reaction is 1.

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 madesome 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 celI, the number n of electrons transferred per redox reaction is 1.

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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(iv) raised from 25 °C to 100 °C? Which of the following would result for any cell if the temperature was A. The cell potential would not change at all B. The cell potential would increase slightly C. The cell potential would decrease slightly D. It is impossible to determine. E. It would depend on the nature of the electrodes used.
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:
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Based on the sign of the standard cell potential, Eel, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Pb2*(aq) + H2(g) - Pb(s) + 2 H*(aq) Ni?*(aq) + s? (aq) Ni(s)+S(s) Al3+(aq) + 3 Na(s) → Al(s) + 3 Na*(aq)
Inert metal electrodes, such as platinum and gold, generate an electrode potential that responds to the redox reaction occurring on the metal surfaces - this type of electrode is called a reference electrode. Is the above information true or false? Explain with reasons.
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.
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 certain metal M forms a soluble nitrate salt M(NO,).. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M (NO,), and 2 the right half cell with a 150. 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 35.0 °C. O left x10 Which electrode will be positive? 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.
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
8:51 AM Mon Dec 5 = S BIOL 286 E B Lecture Pow... Bb Lecture Pow... O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free... cell A 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 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. C 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. n 1 AA 1 1 Explanation 142. kJ/mol O calculated quantities (Check the box next to any that are wrong.) AG - 50. kJ/mol O - 46. kJ/mol O Check www-awu.aleks.com K 24 7.54 x 10 O…
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
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