11. What is the standard cell potential (E°cen) for a galvanic cell constructed fromthese two half-cells?Cr"(aq) + 3e --> Zn(s);E° = - 0.74 V;Cu2*(aq) + 2e --> Cu(s);E° = + 0.34 V;(The cell reaction is: 2Cr(s) + 3Cu2 (aq) --> 2Cr3*(aq) + 3Cu(s)(A) 0.40 V(B) 0.46 V(C) 2.50 V(D) 1.08 V

The cell reaction taking place is given as, => 2 Cr (s) + 3 Cu2+ (aq) ------> 2 Cr3+ (aq) + 3…

11. What is the standard cell potential (E°cen) for a galvanic cell constructed from these two half-cells? Cr"(aq) + 3e --> Zn(s); E° = - 0.74 V; Cu?"(aq) + 2e --> Cu(s): E° = + 0.34 V; (The cell reaction is: 2Cr(s) + 3Cu2 (aq) --> 2Cr3 (aq) + 3Cu(s) (A) 0.40 V (B) 0.46 V (C) 2.50 V (D) 1.08 V

11. What is the standard cell potential (E°cen) for a galvanic cell constructed from these two half-cells? Cr"(aq) + 3e --> Zn(s); E° = - 0.74 V; Cu?"(aq) + 2e --> Cu(s): E° = + 0.34 V; (The cell reaction is: 2Cr(s) + 3Cu2 (aq) --> 2Cr3 (aq) + 3Cu(s) (A) 0.40 V (B) 0.46 V (C) 2.50 V (D) 1.08 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...

See similar textbooks

Related questions

Q: For the cell shown, the measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H, (g. 0.817…

A: Given cell notation is : Pt (s) |H2 (g, 0.817 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd (s)…

Q: 3.33 Calculate the standard free energy change for the follow- ing reactions using the standard cell…

Q: The cell potential of this electrochemical cell depends on the gold concentration in the cathode…

Q: Enter your answer in the provided box. of the following cell is 0.835 V, what is the pH in the anode…

A: To find pH

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: Consider a galvanic cell with the cell notation below. Al(s) | Al3*(aq) || Cr³*(aq), Cr2*(aq) |…

A: Galvanic cell: the cell in which chemical energy is converted into electrical energy From…

Q: (a) Draw the schematic diagram of the Galvanic cell made from the above with appropriate sign…

A: Redox reaction is that type of reaction where oxidation and reduction take place simultaneously.…

Q: 7) A galvanic cell is being made of iron & chromium. The standard reduction potentials are: Fe^2+…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

Q: For the cell shown, the measured cell potential, Ecell, is -0.3509 V at 25 °C. Pt(s) | H₂(g. 0.773…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

Q: In a galvanic cell, the cathode consists of a Ag*(1.00 M)| Ag half-cell. The anode is a platinum…

A: Given: Concentration of benzoic acid = 0.10 M Concentration of benzoate ion = 0.050 M Measured cell…

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s) + 2 H+(aq) ⇔ Ni+2(aq) + H2 (g) Ecello = 0.23…

Q: 6. Balance each skeleton reaction, use Appendix D to calcu- late Ell, and state whether the reaction…

Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

A: An electrolytic cell is a cell which requires an outside electrical source to initiate the redox…

Q: A galvanic cell is constructed using two half-cells in standard state: Al|Al3+ and Ni|Ni+2 Al3+(aq)…

A: To find out the standard cell potential, first check out which species are oxidized and reduced.…

Q: ) Determine the cell potential, Eo, for an electrochemical cell described by the following cell…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V 2H"(aq) +…

A: To solve this problem we will use the given reduction potential of each species .

Q: 11.)

A: We have given that From representation of the cell reaction Oxidation half reaction : Zn(s)…

Q: What is E°cell for the following electrochemical cell? (assume that Pt is an inert electrode) Al |…

A: Using standard reduction potentials , we will calculate E°cell .

Q: Calculate the standard cell potential, E°cell, for the following reaction, and indicate if the…

A: We are given a redox reaction happening in an electrochemical reaction. The oxidation half-reaction…

Q: What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2…

A: Given : half cell reaction Tip : cell having higher value of reduction potential will reduced

Q: Calculate the non-standard cell potential (in V) for the following reaction at 94.68 °C with the…

Q: (aq) + Sn (aq) 11. Calculate the cell potential of a cell operating with the following reaction at…

A: Q 11) cell potential E = - 2.435 V Q 12) Concentration of Ni2+ = 1.832 x 10-5

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: onsider the following half-cells: (1) AgCl(s) | Ag(s), Cl–(aq) E°red =…

A: The given half cells are: (1) AgCl(s) | Ag(s), Cl–(aq) E°red = +0.22 V…

Q: The following electrochemical cell was constructed at 298 K. C. Co(s)CoSO4j|NISO4NI(s) E° Co2*Co =…

Q: E°cell = 1.66 V for the following cell reaction: P4(8) + 3OH´(aq) + 3H2O(1) → PH3(g) + 3H2PO2¯(aq)…

Q: Consider the following half-reactions: Half-reaction E° (V) Br,(1) + 2e → 2Br (aq) |1.080V Co2+…

Q: A voltaic cell employs the following redox reaction: Sn²+ (aq) + Mn (s) → Sn (s) + Mn²+ (aq) which…

A: The cell potential of the electrochemical cell is: Ecello=Ecathodeo-Eanodeo…

Q: G For the cell shown, the measured cell potential, Ecell, is -0.3625 V at 25 °C. Pt(s) | H₂(g, 0.721…

A: At anode : oxidation occurs , oxidation half reaction is H2 (g) → 2H+ (aq) + 2e- ; E°red = 0.00…

Q: Consider the following half-reactions: Half-reaction E° (V) 1(s) + 2e 21(aq) 0.535V Cd2*(aq) + 2e →…

A: Here to identify the oxidizing and reducing power, we will consider the reduction potential of each…

Q: The following reaction occurs in an electrochemical cell: 3 HCIO,(aq) + 2 Cr³* (aq) + 12 H2O(e) → 3…

A: Given: The concentration of Cr2O72-, HClO2, and [HClO] is 0.80 M, 0.15 M and 0.20 M, respectively.…

Q: For the cell shown, the measured cell potential, Ecell, is –0.3525 V at 25 °C. Pt(s) | H,(g, 0.851…

A: The cell given is, Given: Ecell = -0.3525 V Temperature = 25 oC And the half-reactions are,

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V PH2=0.857atm Concentration of Cd2+=1.00M

Q: Using standard reduction potentials, calculatethe standard emf for each of the following…

A: (a) Cl2(g) + 2 I-(aq)---->2 Cl-(aq) + I2(s) Cl2(g) → 2 Cl- Eₒ = 1.36 , Reduction on cathode 2…

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Consider the following half-reactions: Half-reaction E° (V) 2(s) + 2e 21°(aq) 0.535V Ni2+ "(aq) +…

A: We are given the standard reduction potentials of different half cell reactions. We must know that…

Q: Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is…

Q: In a galvanic cell, the cathode consists of a Ag*(1.00 M)|Ag half-cell. The anode is a platinum…

A: Introduction: Galvanic cell is an electrochemical cell in which currents are generated though…

Q: Given the following standard electrode potentals: Ag°(aq) + e¯ = Ag(s) N,(g) + 5H°(aq) + 4e° =…

A: Consider the given values as; Ag+ aq + e- ⇌ Ag s…

Q: 26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e -->…

Q: If a voltaic cell is created between a S/Sr electrode and a Fe"/Fe electrode, what species is being…

A: In this series the element(electrode) are arrange in their electrode potential value with refrence…

Q: dit: Calculate the cell potential for the following galvanic cell at 25°C: Al(s)| AI3+ (0.0632 M)||…

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which [Cry…

Q: Pt(s) | H,(g, 0.839 atm) | H*(aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) balanced reduction half-reactions…

A: Given : We have to calculate concentration of hydronium ion.

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

11. What is the standard cell potential (E°cen) for a galvanic cell constructed from
these two half-cells?
Cr"(aq) + 3e --> Zn(s);
E° = - 0.74 V;
Cu2*(aq) + 2e --> Cu(s);
E° = + 0.34 V;
(The cell reaction is: 2Cr(s) + 3Cu2 (aq) --> 2Cr3*(aq) + 3Cu(s)
(A) 0.40 V
(B) 0.46 V
(C) 2.50 V
(D) 1.08 V

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)
1 2 B A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2(aq) + 2e Co(s) E° -0.28 volt; Cd2+ (aq) + 2e-Cd(s) E°--0.42 volt. What is the standard free energy change in kJ for the cell reaction of this galvanic cell? Report your answer in whole number. Do not put unit in your answer. Type your answer...
Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e → Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 V
Kindly write the sol.n
(a) Define molar conductivity of a substance and describe how for weak and strong electrolytes, molar conductivity changes with concentration of solute. How is such change explained?(b) A voltaic cell is set up at 25 °C with the following half-cells:Ag+(0.001 M) | Ag and Cu2+(0.10 M) | Cu What would be the voltage of this cell?(E0cell = 0 .46 V)
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
A galvanic cell is constructed in which the overall reac- tion is Cr,O} (aq) + 14 H¿O*(aq) + 6 I (aq) → 2 Cr* (aq) 1 3 I,(s) | 21 H,0(€) (a) Calculate AE° for this cell. (b) At pH 0, with [C»O3¯] = 1.5 M and [I-] = 0.40 M, the cell potential is found to equal 0.87 V. Calculate the concentration of Cr³*(aq) in the cell.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (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. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H" (aq)+ 5Co (s) → L, (s)+ 6H,0 (1)+ 5Co" (aq) Suppose the cell is prepared with 6.10 M IO, and 1.61 M H' in one half-cell and 7.06 M Co 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. х10
If the half-cell, Ag(S2O3)2 3- (0.00753 M), Na2S2O3 (0.1439 M) | Ag, is the right-hand electrode in a galvanic cell with a SHE on the left (a) write the full shorthand notation of the electrochemical cells; (b) Given the formation constant, ?2, of Ag(S2O3)2 3- = 1.62x1013 , calculate the cell potential; (c) If the cell were shorted, indicate whether the Ag(S2O3)2 3- , Na2S2O3| Ag electrode would act as an anode or a cathode