Considering that the half-reaction Cr3+(aq) + 3e + Cr(s) has a standard reduction potential of -0.74 V and Ni2+(aq) + 2e + Ni(s) has -0.25 V, which among the following is most likely to become the anode? O Cr(s) O c3*(aq) O N2*(aq) O Ni(s) O none of the choices

Considering that the half-reaction Cr3+(aq) + 3e + Cr(s) has a standard reduction potential of -0.74 V and Ni2+(aq) + 2e + Ni(s) has -0.25 V, which among the following is most likely to become the anode? O Cr(s) O c3(aq) O N2(aq) O Ni(s) O none of the choices

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: If a redox reaction occured with the 2 redox couples provided below, which species would be the…

A: Reducing agent is the substance that reduces the other species and itself gets oxidized.

Q: Calculate Eº, Gº, and K at 25 °C for the reaction: 2MnO4 (aq) + 4H+ (aq) + Cl₂(g) (Use: CIO3 to Cl₂…

A: The given reaction is - 4MnO4-aq + 4H+aq + Cl2g → 2Mn2+aq + 2ClO3-aq + 2H2O Oxidation -…

Q: 4. A voltaic cell that uses the following reaction has a measured emf of 1.19 V under standard…

A: By taking the values of electrode potential of the two half cells, the total emf of the…

Q: Consider the following half-reactions: Cl2(9) + 2e - 2cF (ag) = 1. %3D I2(9) + 2e - → 21 (aq) E, =…

A: From given data , based on the E° value given for the half actions we can predict the strongest…

Q: 5. Balance the following redox reaction in BASIC solution: + Br' (aq) → MnO2(aq) + BrO3" (aq) MnO4…

A: While balancing of chemical reaction ,we balance 1) Mass balance : No of atom of respective atom…

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

Q: 31. Calculate AG° for the following galvanic cell: Mn(s) | Mn²"(aq) || Fe"(aq) [Fe(s), given these…

Q: (e) O2(8) → H20(1) (basic solution) (f) Mn²*(aq) → MnO2(s) (basic solution) (g) Cr(OH)3(s) –→…

A: Oxidation - it is the loss of electrons with increase in the oxidation sate. Reduction - it is the…

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

Q: Calculate the Kf of Ag(NH3)2+ from

A: For kf, the reactions arrangement - Ag+aq+e⇔Ags...E∘=0.80 VAgs + 2NH3aq ⇔AgNH32++e-...E∘=-0.37VAdd…

Q: Balance the following redox equations. All occur in basic solutions. (A) Al(s) + H2O(l) -->…

A: 1) Write the redox equations Al(s) + H2O(l) -->…

Q: at a temperature of 25 ° C the galvanic element Pt | ClO3- 0,001M, Cl- 0,01M pH = 3 || Mn2 + 0.0001M…

Q: 21.31 Balance each ske whether the reaction is (a) Co(s) + H* (aq) (b) Mn2 (aq) + Br,(1) (c)…

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

A: Answer:In an electrolytic cell oxidation always occurs at anode and reduction always at cathode, so…

Q: FORLAD 4 Consider the redox reaction where Ag+ (aq) is oxidized to Ago (s) (E° 0x = -1.77 v) and…

Q: Given the electrochemical reaction shown, what is the E of the reaction? Mg | Mg2*(ag) || Zn2* (aq)…

Q: 7. Calculate AG° for the following galvanic cell Zn(s) | Zn²*(aq) || Fo2*(aq) IFe(s) given these…

A: The standard electrode potential of a Galvanic cell is given by the formula E° = E°(cathode) -…

Q: 4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and…

Q: Metals like sodium, potassium, calcium and magnesium are extracted by electrolysis of their…

Q: Voitmeter Cr(s) Ag(s) Cr*(aq) Ag (aq) 1) The Galvanic cell pictured above is constructed with…

Q: 3. How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn²+ (aq) if the…

Q: For the galvanic cell at 298 K 2Cr(s) + 3NI2+(aq) 20r3+(aq) + 3Ni(s) cell = 0.51 V What is the…

Q: Consider the following half-reactions: Half-reaction Ag+ (aq) + e Co2+ (aq) + 2e™ Cr3+ (aq) + 3e E°…

A: Here we are required to arrange the species on increasing order of strength of oxidizing agent

Q: (a) Write down the overall reaction for the formation of the complex ion [Zn(NH:)-]²*(aq) from its…

Q: If a redox reaction occured with the 2 redox couples provided below, which species would be the…

A: Correct answer is (d) HOOCCOOH(aq) . HOOCCOOH(aq) will be reducing agent in the spontaneous cell…

Q: Complete and balance the following half-reaction in basic solution. MnO4-(aq) +C2O2-2(aq) (->)…

Q: Balance the following redox reaction in basic solution. SO;²- (aq) + Cr2O,7-(aq) → Cr³*(aq)+…

A: Given that : We have to balance the following redox reaction in basic solution : SO32-(aq) +…

Q: [Réview Topics] [References) Use the half-reactions shown below to answer the following questions.…

A: The species which has higher reduction potential that is reduced and oxidize other which has lower…

Q: 4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and…

A: Step 1:

Q: [References] Using values from the table of standard reduction potentials, calculate the standard…

A: We can solve this problem by using following equation ∆G° = -n×F×E° n = change no of electrons F =…

Q: [4] Balance the following redox reaction in basic solution. SO;2- (aq)+ Cr207 (aq) → Cr*(aq) +…

A: Redox reaction is combination of both oxidation and reduction

Q: Sketch the galvanic element diagram consisting of the following two half-elements Cu2O | Cu, in…

Q: Use the standard reduction potentials located in the "Tables' linked above to calculate the standard…

A: Given :

Q: [3] Given the Standard Reduction Potentials at 25°C, Mn++2e Mn E° =-1.185V and Hg+2e - Hg E° =…

A: 1- When the standard reduction potential is negative that means it is an oxidation half reaction and…

Q: (a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing…

A: An oxidizing agent are the agents that help in removal of electrons from other reactants. We can…

Q: calculate the potential of platinum elctrode emersed in a solution 0.0613 M in k4Fe(CN)6 and…

A: The concentration of k4Fe(CN)6=0.0613 M The concentration of k3Fe(CN)6=0.00669 M The oxidation…

Q: How many electrons are transferred in the redox reaction taking place in basic solution: Cr(s) +…

A: The given reaction is, Cr(s) +ClO4-(aq) →ClO3-(aq) + Cr3+(aq) On the reactant side, The oxidation…

Q: Using the standard reduction potentials, Pb4 (aq) + 2e- => Pb(s), E° = -0.13 V Fe(aq) + 2e- =>…

A: A chemical reaction in which loss of electron and gain of electron takes place simultaneously is…

Q: Complete and balance the following redox reaction in basic solution Cr20,2 (aq) + Hg(1) → Hg2* (aq)…

A: 1- Oxidation Half reaction : Hg(l) -------> Hg2+(aq) + 2e- Multiple with 3 3Hg(l) ------>…

Q: It is requested: a) The direction of the current

A: Galvanic cells: the devices in which chemical energy is converted into electrical energy Redox…

Q: Complete and balance the following redox reaction in basic solution Pb2+(aq) +IO3-(aq) ---> PbO2(s)…

Q: Complete and balance the following redox reaction in acidic solution As(s) + 10 H*(aq) → H3ASO,(aq)…

A: Complete and balanced the redox reaction under acidic condition ----

Q: Consider the half-reaction Ag+(aq) + e------>Ag(s).(a) Which of the lines in the following…

A: (a) The given reaction is, Ag+(aq) + e- ---> Ag(s) Ered = Eo - ( 0.0591/n ) log ( 1/ [Ag+] E red…

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

Considering that the half-reaction Cr3+(aq) + 3e + Cr(s) has a standard reduction potential of -0.74 V and Ni2+(aq) + 2e + Ni(s) has -0.25 V, which among
the following is most likely to become the anode?
O Cr(s)
O cr3*(aq)
O Ni2*(aq)
O Ni(s)
O none of the choices

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

Can you help me solve 19.85?
If the standard voltage of the reaction of Cu(s) with Ag*(aq) is 0.46 V, what is the standard gibbs energy of reaction? O -89 kJ O +46 kJ O -56 kJ O -150 kJ
Complete and balance the following redox reaction in basic solution: Zn(OH)42- (aq) + As (s) --> Zn (s) + H2AsO4- (aq)
For the following two reduction half-reactions, which will occur at the cathode? a) Fe3+(aq) + e- --> Fe2+(aq) Eo = +0.771 V b) Pt2+(aq) + 2e- --> Pt(s) Eo = +1.20 V
The standard reduction potential E° for the reduction ofpermanganate in acidic solution is +1.51 V. What is thereduction potential for this half-reaction at pH = 5.00? MnO4–(aq) + 8 H+(aq) + 5 e– → Mn2+(aq) + 4 H2O(l)E° = +1.51 V(A) +1.50 V (B) +1.42 V(C) +1.04 V (D) –0.85 V
1. Write balanced redox equations for the following reactions. Show the full balancing process and supply H* and/or H2O as needed to obtain balance. Item g is balanced in basic medium while the rest are in acidic medium. (a) MnO, + VO²+ → Mn²+ + V(OH),+ (b) Iz + H,S(g) →I+S(s) (c) Cr,0,²- + U+ → C²+ + UO,²+ (d) CI¯ + MnO2(s) → Cl2@) + Mn²+ (e) IO,¯ + I¯ –→ 1(aq) (f) IO; + I¯ + Cl¯ → ICl,¯ (g) HPO,²-+ MnO,¯+OH¯→ PO,-+ MnO,²- 2. Identify the oxidizing agent and the reducing agent on the left side of each equation in the previous problem.
Pt(s)|Fe2+(aq),Fe3+(aq)||F-(aq)|F2(g)|C(s) Which is the reducing agent? F2 Fe3+ Fe2+ F-
agent? (a) Ag (aq) 20. Which statement is true considering the following reactions? Sn² (aq) +2e-> Sn (s) E = -0.136 V Fe" (aq) +3e > Fe (s) E = -0.036 V (a) The tin electrode is the cathode and electrons flow from anode to cathode (b) The tin electrode is the cathode and electrons flow from cathode to anode (c) The tin electrode is the anode and electrons flow from anode to cathode (d) The tin electrode is the anode and electrons flow from cathode to anode 21 Which of the following r reser (b) Ag (s) (c) Zn² (aq) (d) Zn (s)
(a) Calculate the emf for the given cell at 25 °C:Cr | Cr3+(0.1 M) || Fe2+ (0.01 M) | Fe [Given: E°Cr3+/Cr = -0.74 V, E°Fe2+/Fe = -0.44 V](b) Calculate the strength of the current required to deposit 1.2 g of magnesium from molten MgCl2 in 1 hour.[1 F = 96,500 C mol-1; Atomic mass: Mg = 24.0]
(a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing agents in strong acid: Ⓒ BrO₂ O Cd²+ O Hg2+ O Co²+ O H₂SO3 ΟΙ O Fe O NO O H₂ O Bi • BrO3 O Cd²+ O Hg2+ O Co²+ O H₂SO3 X X or O Fe O NO O H₂ O Bi BrO3 O Cd²+ O Hg2+ O Co²+ O H₂SO3 I O Fe O NO 10 Hz O Bi (b) Assuming standard conditions, arrange the following in order of increasing strength as reducing agents in strong base: H₂ X X Ⓒ BrO3 O Cd²+ O Hg²+ O Co²+ O H₂SO3 ΟΙ O Fe O NO O H₂ Ο Bi X X © BrO3 O Cd²+ O Hg2+ O Co²+ O H₂SO3 or O Fe O NO O H₂ O Bi X BrO3, Cd²+, Hg2+, Co²+, H₂SO3 I, Fe, NO, H₂, Bi
Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Zn(3)| Zn*r||Cu*|Cu(e) В © Au(s)|Au|| Mn**|Ma(e) 2+ Co(s)| Co*" Fe* |Fe(e)
Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Au() Au"|| Ma* |Ma{e) ® Co(o) Co*| Fc*|Fo(e) B © Za(o)|Za*| cu*|cue)