1. Look at the cell diagram as follows: Co(s) I Co²*(aq) II Cu²*(aq) I Cu*(aq) I Pts) If known E° CO(s) I Co²+ The magnitude of the Gibbs energy and the spontaneity of the reaction in the cell diagram is *(aq)= - 0,28 V dan E° Cu²*(aq) I Cu*(aq) = +0,15 V %3D ........

1. Look at the cell diagram as follows: Co(s) I Co²(aq) II Cu²(aq) I Cu(aq) I Pts) If known E° CO(s) I Co²+ The magnitude of the Gibbs energy and the spontaneity of the reaction in the cell diagram is (aq)= - 0,28 V dan E° Cu²(aq) I Cu(aq) = +0,15 V %3D ........

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: Calculate the standard e.m.f, standard free energy change and equilibrium constant for the following…

A: Answer: Since, Copper is getting oxidized therefore it will be at anode and chlorine is getting…

Q: An electrochemical cell is constructed in which a I2(s)|I(1.00 M) half-cell is connected to an…

A: An electrochemical cell is made up of I2 s|I- 1.00 M and H3O+ aq|H2 1 atm. The measured cell…

Q: Calculate the cell potential for the following reaction and indicate whether it is spontaneous or…

A: using deltaG* to determine where the reaction is spontaneous or non-spontaneous.

Q: Consider a cell consisting of the following two ½ equations, Zn2+ / Zn E0 = - 0.76 Volts Fe2+ / Fe…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: The cell potential was -0.228 V at 25oC and a Fe3+(aq) concentration of 0.162 M. What was the pH of…

A: The Nernst equation for the given cell at 25oC is: Ecell=Ecell∘-0.059nlog Q······(1) Here, Ecell is…

Q: 2Cr3+(aq) + 3Ni(s) Eocell = 0.51 V What is the measured cell potential (Ecell) when…

Q: QUESTION 12 Continue with the last question, the corresponding cell notation is Sn(s) | Cu²+ (aq) ||…

A: The given reaction is Sn (s) + CuSO4 (aq)→ SnSO4 (aq) + Cu (s) To find: Which electrode is acting…

Q: A Zn-Ag Galvanic cell has an Ecell value of 1.536 V. The cell diagram is as blow. Calculate the…

A: This is a simple question of electrochemistry for the application of Nernst equation.

Q: The free energy change for the following reaction at 25 °C, when [H*] = 8.48x10-3 M and [Fe3+] =…

A: The given chemical reaction is

Q: 6. What is E° for the cell Ms)| Mn²"(aq) || Ag'(aq) | Ag(s) ? Standard Redu on Potentials E° (V)…

A: Consider the given cell representation is as follows; Mn s | Mn2+ aq || Ag+ aq | Ag s To determine…

Q: For the galvanic (voltaic) cell Cd²*(aq) + Fe(s) – Cd(s) + Fe²*(aq) (E° = 0.0400 V), what is the…

A: The expression of Nernst equation is shown below: Where; Ecell= cell potential E0cell = standard…

Q: What is the molar concentration of Fe3+(aq) if the cell potential was -0.3792 V and the molar…

A: According to Nernest equation- Ecell = Estdcell - 0.0591/n * log [Product/Reactant] n = No of…

Q: [References] Write the overall cell reaction for the following voltaic cell. Pt|H2 (9) H (ag) || Br2…

Q: a Calculate E° for the following cell: Hg | Hg22+ || Pb4", Pb2+ | Pt You may need to use the…

A: The answer to the following question is-

Q: What is the cell diagram for the spontaneous cell involving the Fe3+(aq) | Fe2*(aq) I Pt(s) (0.771V)…

A: For a spontaneous cell reaction the half cell with greater reduction potential act as cathode while…

Q: Calculate the cell potential for the following concentration cell at 25 °C.…

A: Here the cell represented consists of a cathode and the anode made up of nickel. In the cell…

Q: Given the following reaction MnO4- (aq) + Ag(s) --> Ag+ (aq) + Mn (s) a.) Provide a balanced…

Q: The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s)…

A: This question belongs to Electrochemistry. The condensed cell diagram for the reaction occurring in…

Q: Determine electromotive force for the cell represented by: Fe (s) | FeSO4(0.30 M) ||…

A: The cell given is, => Fe (s) | FeSO4(0.30 M) || KIO3(0.50 M), l2(s), pH 4.0 | Pt(s) In the above…

Q: hat is the standard cell potential of the following electrochemical cell at 25°C: i(s) | NiCl2(aq)…

A: Given-> Ni(s)/NiCl2(aq)//Cu(NO3)2(aq)/Cu(s)

Q: Calculate the cell potential for the following electrochemical cell at 25°C. Sn(s) i Sn2+(aq, 0.022…

A: E°cell= E°(cathode)- E°(anode) [Sn^2+] = 0.022M [Ag^+] =2.7M

Q: Consider a galvanic cell below and calculate the concentration of Au*3 solution. The measured cell…

Q: Calculate the cell potential for a cell at 30°C with a Cu2+ concentration of 0.012 M and a Zn²+…

Q: What is undergoing oxidation in the redox reaction represented by the following cell notation?…

Q: Consider the following half-cells: (1) AgCl(s) | Ag(s), Cl–(aq) E°red = +0.22 V…

A: In this question, we will Identify which combination produces Highest voltage. How we can identify…

Q: What is the expected standard cell potential for the following unbalanced reaction under basic…

A: In the given cell reaction, ferrous ion is oxidized to ferric ion. The oxidation state of iron…

Q: 2Cr(s) + 3Ni²+ (aq) 2Cr³+ (aq) + 3Ni(s) Ecell 0.51V =

A: The given redox reaction is 2 Cr(s) + 3 Ni2+(aq) →2 Cr3+(aq) + 3Ni(s), E°cell = 0.51 V The measured…

Q: According to the following cell notation, which species is undergoing oxidation? Fe(s) | Fe2*(aq) ||…

Q: Calculate the equilibrium constant K, for the following balanced redox reaction at 25oC. (R = 8.31…

A: When a reaction is in equilibrium it has the value of Gibbs free energy change of the reaction as…

Q: Consider the following half-reactions: E° = +2.87 V F2(9) + 2 e ® 2 F'(aq) Cu2*(aq) + 2 e¯ ® Cu(s)…

A: To reduce Al+3 to Al the compound used must have more negative reduction potential than Al+3.

Q: Consider an electrochemical cell with the following cell notation: Fe(s) Fe²+ (aq) (from saturated…

A: Given half cell is Fe(s)|Fe2+(aq) (from Saturated FeCO3) || Fe2+(aq) (0.150 M) | Fe(s) And standard…

Q: 6 What potential, in volts, is developed by the following electrochemical cell at 298 K? AP (0.00100…

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

1. Look at the cell diagram as follows: Co(s) I Co²*(aq) II Cu²*(aq) I Cu*(aq) I Pt(s)
If known E° CO(s) I Co²*(aq) = - 0,28 V dan Eº Cu²*(aq) I Cu*(aq) = +0,15 V
The magnitude of the Gibbs energy and the spontaneity of the reaction in the cell
diagram is
...
2. NazS207 + TIO2= N22SO4 + TIOSO4
The acid-base theory that underlies the TiO2 compound as a basic species is
a. Usanovich
b. Lewis
c. Bronsted-Lowry
d. Lux-Flood

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

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

Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
42 only
e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
Determine electromotive force for the cell represented by: Fe (s) | FeSO4(0.30 M) || KIO3(0.50 M), l2(s), pH 4.0 | Pt(s) Given: Fe2+ + 2 e --------- Fe (s) Eo = - 0.44 Fe3+ + e ------ Fe2+ Eo = 0.771 V IO3- + 6 H+ + 5e ------ ½ I2(s) + 3 H2O (l) E0 = 1.210 V A. 1.346 V B. 0.166 V C. 1.376 V D. 0.498 V E. 1.660 V
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5
1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential 2) Calculate the free energy change and the cell potential for the reaction at 298.0 K if all reactants are at 2.00 M and/or 2.00 atm and all products are at 0.0100 M and/or 0.0100 atm
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
In the electrochemical cell shown here, the concentrations of Mn2+ and Cr3+ are 1.5x10-5 and 0.25 mol L-1, respectively. What is the cell potential? = E 0.0257 V -InQ KNO, Mn Mn(NO3)2 Cr(NO3)3 Mn* (aq) + 2e 2 Mn(s) E° =-1.18 V Cr* (aq) + 3e¯ 2 Cr(s) E° =-0.74 V
Consider the following reaction at 298K. Cu²* (aq) + Fe²* (aq) Cu* (aq) + Fe* (aq) Which of the following statements are correct? Choose all that apply. On-1 mol electrons OK>1 AG° <0 E° cell 0 The reaction is reactant-favored.