A favorable REDOX reaction... O has a positive Ecell value and a negative delta G O a negative Ecell value and a positive delta G O a negative Ecell value and a negative delta G O a positive Ecell value and a positive delta G

A favorable REDOX reaction... O has a positive Ecell value and a negative delta G O a negative Ecell value and a positive delta G O a negative Ecell value and a negative delta G O a positive Ecell value and a positive delta G

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 26Q: In theory, most metals should easily corrode in air. Why? A group of metals called the noble metals...

See similar textbooks

Related questions

Q: 23). Can nickel metal (Ni) reduces Cut2 to copper metal or Cu? (hint. will the reaction be…

A: The reaction taking place will be Ni + Cu2+ -------> Cu + Ni2+ Hence the Ni will be oxidised to…

Q: The best true statement for voltaic cell? E for the cell is always positive. O The standard…

A: Electrochemical cell are those cell which converts electrical energy to chemical energy or vice…

Q: 21.31 Balance each skeleton reaction, whether the reaction is spontaneous: Co2+(aq) + MnO (ac Hg2…

Q: Vrite a balanced =quation for the alf-reaction that appens at the athode. Vrite a balanced equation…

A: Zn (s) ----> Zn+2(aq) + 2e HNO2(aq) + H+ + e- ----> NO(g) + H2O(l)

Q: If the Δ°G value is positive, can the reaction be spontaneous in a cell (ΔG negative)? How, why or…

A: Given : ΔG° is positive for the cell.

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: Calculate the emf of the following concentration cell: 2+ Mg(s)| Mg*(0.35 M) || Mg*(0.59 M) |Mg(s)…

A: Given, Mg(s) | Mg2+(0.35 M) || Mg2+(0.59 M) | Mg(s)

Q: A current of 3.22 A is passed through a Ni(NO,), solution. How long, in hours, would this current…

A: We have to calculate the time required.

Q: otentials. 2 +2H2O + 4e --> 40H Enote = 0.401V a2+ 2e ----> Ca Enote = -2.868 alculate the maximum…

Q: se standard reduction potentials to calculate the standard free energy change (AG") for the reaction…

A: We have to find∆G

Q: Calolate the Standard emf of a cell that uses Ag/Ag* and Al/AI+ Half cell reachons.

A: The electrode which has higher reduction potential acts as a cathode and the electrode with lower…

Q: Cathode is ... terminal. * Negative. Positive.

Q: Which of the following statement/s is/are false? All spontaneous oxidation-reduction reactions have…

Q: Oxidation is O a. Loss of electron O b. gain of electron Oc. gain and then lose of electron Od. loss…

A: Oxidation is process or result of oxidizing or being oxidized. If oxygen is being added to any…

Q: The KTH value for a redox reaction is equal to 3.4 x 1015. Calculate the value of ΔGo ΔGo =…

A: The standard Gibbs free energy ∆G∘ for the redox reaction is calculated using the following…

Q: Using this table of standard reduction potentials determine which of the following is the strongest…

A: The species which oxidises itself and reduce other is known as reducing agent.

Q: (b) Given the overall equation a redox reaction alongside the standard reduction potentials, E°:…

Q: Ag + e- ---- > Ag (s) - This reaction is most likely to take place at the anode O cathode either…

A: A question based on electrochemistry, which is to be accomplished.

Q: dation occurs at the negative anode and nonspontaneous read dation occurs at the positive cathode…

A: Galvanic cells, also known as voltaic cells, are electrochemical cells in which spontaneous…

Q: A reaction with a higher potential is more likely to occur. True O False

A: Answer: Electrochemical is the type of cell in which chemical energy gets converted into electrical…

Q: Given the reduction reaction and reduction potentials. Which of the reactions (a-e) are spontaneous?…

A: ΔG is negative for a spontaneous reaction. Therefore, the value of electromotive force(emf) or…

Q: Consider the following reduction half-reactions and the corresponding standard reduction potentials,…

A: Given that : We have to rank following the reducing agents in terms of increasing strength, i.e.…

Q: List from strongest to

A: EoLi+/Li = - 3.04 V EoNa+/Na = - 2.71 V EoMg+2/Mg = - 2.37 V Hence in the given 3…

Q: Batteries have a negative and positive end. O True O False

A: Batteries have three parts ,an anode (-),a cathode (+),and the electrolyte.the cathode and anode…

Q: Which is correct for a redox reaction where the standard electrode potential is negative? AGe=-nFEe…

Q: Remember that the lower an element's chemical potential, the easier it is to oxidize. Using…

A: Oxidation reaction- Increase in oxidation number due to loss of electrons. Lower an elements…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Answer

Q: n the process of electroplating, anions are reduced at the anode and be deposited on the cathode as…

A: Electroplating is a process of creating a metal layer on solid species by using the concept of…

Q: Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard…

Q: 9. How many grams of Cu are plated out from a CuSO4 solution by a current of 7.8 amps flowing for…

A: We have to predict the mass of Cu deposited.

Q: Standard reduction potential Zn²+ (aq) + 2e → Zn (s) O₂(g) + 4H+ + 4e →2H₂O(l) Calculate Eºcell for…

A: Since O2(g) has higher reduction potential of 1.066 V, it will undergo reduction to H2O(l), and…

Q: Suppose that the concentration of Cat outside the cell is 10 and inside the cell is 0.01 mmol/liter.…

A: Given, [Ca2+]outside= 10 mmolL[Ca2+]inside = 0.01mmolL membrane voltage = +87 mV

Q: For the re the followi MnO4 + (a) What i Mn in MnC

A: Oxidation number is the partial or imaginary charge present on an atom in the compound. a) +7 b) +4…

Q: I, E°cell, for the reaction?

Q: An electrochemical cell with the given line notation was constructed. S.C.E. || cell solution |…

Q: ow many Faraday is needed to deposit 5 moles of Aluminium (Al) from AlCl3 solution using…

A: According to Faraday law:- when the same quantity of electricity is passed through a solution of…

Q: volt Battery In the electrolysis of water, which electrode(s) is(are) active electrodes? both…

A: The solution is given below -

Q: Cr3+(aq) + 3e- à Cr(s) -0.763 V Au+(aq) + e- à Au(s)…

A: Given reactions are : Cr3+(aq) + 3e- -------------> Cr(s) E0 = -0.763…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

Q: (Q87) If the reduction potential of the species being oxidized is less than that of the species…

A: Here we are required to find whether the electrochemical cell reaction is spontaneous and non…

Q: In a reaction between Fe + CUSO4 (aq) FeSO4(aq) CU(s) + Select one: O a. copper gains electron O b.…

A: In the redox reaction between iron and copper sulfate the half reactions are as follows: oxidation…

Q: 5. The a spontaneous redox reaction in a voltaic cell has a Ecell and a negative (use positive or…

Q: 2+ 3+ The conversion of Fe to Fe is O a. Oxidation O b. substation OC. Redox O d. Reduction

A: Conversation of Fe2+ to Fe3+ occurs when Fe2+ releases one electron from outermost electron shell.

Q: Which is false: a. Cu oxidation is spontaneous at all T. b.Mg is the most stable among the given…

A: Given diagram is : Which is false: a. Cu oxidation is spontaneous at all T. b. Mg is the most…

Q: Choose all of the statements from below which are true about strengths of oxidants and reductants. O…

Q: Aluminum has a mor v [Select] positive negative reduction potential than zinc. To work better as a s…

A: The reduction potential along with the reduction reaction of Zinc and Aluminium are Al3+ + 3 e-…

Q: Which of the following statements is correct? Circle all that apply. Explain. A. An E° value of…

Q: Metal ENGGMATH GMATH ENGGCHEM GRVA FIT HW What metal is used as the cathode in the experiment? O FIT…

A: As we know that which is having high standard electrode potential that is act as cathode. Because…

Q: Calculate the emf for the following reaction. Will the reaction occur spontaneously at 25°C, given…

A: Given- [Fe2+]=0.400M [Cd2+]=0.00790M

Question

A favorable REDOX reaction....
has a positive Ecell value and a negative delta G
O a negative Ecell value and a positive delta G
O a negative Ecell value and a negative delta G
O a positive Ecell value and a positive delta G

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 with 2 images

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

Calculate G for each of the following reactions from the equilibrium constant at the temperature given. (a) N2(g)+O2(g)2NO(g)T=2000CKp=4.1104 (b) H2(g)+I2(g)2HI(g)T=400CKp=50.0 (c) CO2(g)+H2(g)CO(g)+H2O(g)T=980CKp=1.67 (d) CaCO3(s)CaO(s)+CO2(g)T=900CKp=1.04 (e) HF(aq)+H2O(l)H3O+(aq)+F(aq)T=25CKp=7.2104 (f) AgBr(s)Ag++Br(aq)T=25CKp=3.31013
How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range corresponds to basic solutions? Why is pH = 7.00 considered neutral? When the pH of a solution changes by one unit, by what factor does the hydrogen ion concentration change in the solution? How is pOH defined? How arc pH and pOH for a given solution related? Explain.
In theory, most metals should easily corrode in air. Why? A group of metals called the noble metals are relatively difficult to corrode in air. Some noble metals include gold, platinum, and silver. Reference Table 17-1 to come up with a possible reason why the noble metals are relatively difficult to corrode.
What is G for the following reaction? 2Br(aq)+Cl2(g)Br2(l)+2Cl(aq) Use data given in Table 19.1.
Consider the following galvanic cell: Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow.
Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
. To obtain useful electrical energy from an oxidation-reduction process, we must set up the reaction in such a way that the Oxidation half-reaction and the reduction half-reaction are physically one _____another.
What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?