Which of the following statement/s is/are false?V All spontaneous oxidation-reduction reactions have an E°,cellwitha negative sign.O The anode of a battery is the site of reduction and is negative.O Standard conditions for electrochemical cells are a concentration of 1.0 M fordissolved species and 1.0 atm pressure for gases.Oxidation always occurs at the anode part of a spontaneous cell.The potential of the cell does not change with temperature.

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Answered: Which of the following statement/s…

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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Consider the following electrochemical cell: Co*2 (0.038 M) | Co(s) || SHE (E°Co/Co = - 0.277 V) Which of the statement(s) is / are correct ? |- Ecell for this reaction is -0.235 V Il- Keq for this reaction is 1.70 x 10-11 III- Ecell < 0, therefore the cell is spontaneous Select one: O a. I and II O b. I and II Oc. Only II O d. I, Il and III O' e. Only I Of. Only II O g. Il and II
14. Calculate the equilibrium constant K, for the following balanced redox reaction at 25oC. (R = 8.31 J/mol.K). Pb2+(aq) + 2Ag(s) → Pb(s) + Ag+(aq) given the following standard redox potentials: Pb2+(aq) + 2e- ⟶⟶ Pb(s) E0 = -0.13 V Ag+(aq) + e-⟶⟶ Ag(s) E0 = 0.80 V A. 72.47 B. 3 x 1031 C. 0.93 D. 4.9 x 1011 E. 3 x 10-32
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
A redox reaction used in an electrochemical cell has a negative standard free energy change, AGxn- Which statement about the redox reaction is true? O Ecel is positive; K 1 E'cel is negative; K 1 'cell
im a student plz help
nge in 5 on 6 O tion 7 stion 8 estion 9 " Question 10 11 Submit Use the References to access important values if needed for this question. A Fe Fe²+ || Cd²+ | Cd galvanic cell is constructed in which the standard cell voltage is 3.70×10:2 V. Calculate the free energy change at 25°C when 0.863 g of Cd plates out, if all concentrations remain at their standard value of 1 M throughout the process. What is the maximum amount of work that could be done by the cell on its surroundings during this experiment? Submit Answer 5 question attempts remaining AGⓇ Maximum work= X A
The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) → 2 H₂O(l) K = 1.34 x 1083 (a) Calculate and AG at 298 K for the fuel-cell reaction. V k] 80 AGO (b) Predict the signs of AH° and AS for the fuel-cell reaction. AH°: O positive. O negative AS°: positive O negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. Since AS is ---Select---, as T increases, AG becomes more ---Select--- . Therefore, the maximum work obtained will ---Select--- as T increases. ASK YOUR TEACH
Consider an electrochemical cell operating under standard conditions and at 25 °C. One half cell is the standard hydrogen electrode and the other contains dichromate ions and chromium(III) ions in an acidified solution. When the cell operates, the value of A G is O a. 770 x 105 J O b.257 x 105 J O C. 3.85 x 105J Od. 770 x 105J O e..257 x 105 J Of. 3.85 x 105 J O g. None of the above.
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
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. • 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
10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V с. 0.60 V d. -0.60 V e. 0.095 V enstant fr ther

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