DQuestion 1AP" (aq) + 3eMg (aq) + 2eMgMg(NO₂)₂The electrons would flow [Select]The [Select]Al(s)Mg(s)Question 2Voltmetersalt bridgeGiven the electrochemical cell in the picture:In the balanced cell reaction, the number of electrons transferred is [Select]AgAgNO,The standard (assuming 1 M concentrations) cell potential is [Select]-1.67-2.356The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select]If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take [Select]If the concentrations were changed to [Mg2+] = 5.00 M and (Ag*] = 0.0100 M, the cell potential would then be [Select]lyje Question 1DMgThe electrons would flow [Select)Mg(NO₂)Th✓ [Select]VoltmeterGiven the electrochemical cell in the picture:In the balanced cell reaction, the number of electrons transferred is [Select]Ifsalt bridgeQuestion 2AgThe standard (assuming 1 M concentrations) cell potential is [Select]AgNO,The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select]silver electrode gains mass because the silver is oxidizedmagnesium electrode gains mass because the magnesium is oxidizedmagnesium electrode gains mass because the magnesium ions are reducedsilver electrode gains mass because the silver ions are reducedIf the concentrations were changed to [Mg15.00 M and (Ag] 0.0100 M, the cell potential would then be [Select]current is measured to be a constant 1.250 A, it would take [Select]

In a given electrochemical cell, at anode, the oxidation occurs while reduction happens at the…

Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred is [Select] The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential is [Select] The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select] The [Select] If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take [Select] If the concentrations were changed to [Mg] -5.00 M and [Ag] -0.0100 M, the cell potential would then be [Select]

Given the electrochemical cell in the picture: In the balanced cell reaction, the number of electrons transferred is [Select] The electrons would flow [Select] The standard (assuming 1 M concentrations) cell potential is [Select] The change in standard Gibbs' Energy, AG, for the overall reaction would be [Select] The [Select] If the voltmeter was replaced with a resistor (that allows current to flow) and the current is measured to be a constant 1.250 A, it would take [Select] If the concentrations were changed to [Mg] -5.00 M and [Ag] -0.0100 M, the cell potential would then be [Select]

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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Write the cell notation based on the description of the following information: Iron (III) ions are reduced to iron (II) ions in the presence of platinum electrode, and tin is oxidized to tin (II) under standard conditions.
A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for 15.5 h. What mass of Mg is produced? g
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.
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current of 1.97 A to plate 0.0672 g of metal from a solution containing M2(S04)3 (Round off the final answer to TWO decimal places. Do not include the unit.) A Moving to another question will save this response. «< Question 6 of 12 »
Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness.
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
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 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. 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 U calculated quantities (Check the box next to any that are wrong.) AGⓇ -117. kJ/mol - 129. kJ/mol 112. kJ/mol K 3.18 × 10 2.51 X 10 4.18 × 10 21 - 23 19 0 E 1.21 V - 1.34 V 1.16 V
mass of an rolysis product from the applied... When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PbSO,) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 16.0 A is fed into a car battery for 47.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Be sure your answer has a unit symbol and the correct number of significant digits. Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center o search 99+ DE
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
bew DARGERS Determine the thermodynamic equilibrium constant K for a voltaic cell made of a Ag strip and an Al strip immersed in 1.0 M aqueous AgNO3 and Al(NO3)3 solutions, respectively, at 25.00°C, with all other cell components in place. (Use Table 18.3 for your standard cell potentials.) Type your numeric answer and submit Hint Equation 18.8 in Section 18.3.1 relates cell voltage to AG. SOPINIOANE Cat 0 Cannot be empty HE HIG X