24.Given the following half-cell reactions:2+Fe²+ (aq) + 2e¯¯ Fe (s)Eº3+Cr³+ (aq) + 3e-Cr (s)a. +1.18 Vb. -0.30 VC.-1.18 VFe²+ (Aq)1M-0.44 V= -0.74 VFeCrCp 3+d. +0.30 Ve. +1.34 V(Aq)At 25°C, the initial cell voltage of the cell shown in the diagram above is1M

Answer:- This question is answered by using the simple concept of calculation of standard cell…

24. Given the following half-cell reactions: 2+ Fe²+ (aq) + 2e Fe (s) Cr³+ (aq) + 3e¯- → Cr (s) a. +1.18 V b. -0.30 V C. -1.18 V 2+ Fe (Aq) 1M E = -0.44 V E = -0.74 V Fe Cr Cr³+ (aq) 1M At 25°C, the initial cell voltage of the cell shown in the diagram above is d. +0.30 V e. +1.34 V

24. Given the following half-cell reactions: 2+ Fe²+ (aq) + 2e Fe (s) Cr³+ (aq) + 3e¯- → Cr (s) a. +1.18 V b. -0.30 V C. -1.18 V 2+ Fe (Aq) 1M E = -0.44 V E = -0.74 V Fe Cr Cr³+ (aq) 1M At 25°C, the initial cell voltage of the cell shown in the diagram above is d. +0.30 V e. +1.34 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: half-reaction standard reduction potential 2+ Zn (aq)+2e Zn(s) E=-0.763 V red HNO,(aq)+H (aq)+e…

A: Using concept of galvanic cell we can solve this problem. From given half cell data.

Q: below Ba2+ + 2e --- Ba(s) E° = - 2.91 v Mg2+ + 2e --- Mg(s) E° = -2.38 v Fe2+ + 2e --- Fe(s) E°…

A: Reduction occur at cathode and oxidation occur at anode. E°cell = E° reduction + E°Oxiation

Q: Given the following electrochemical cell, calculate the potential for the cell in which the…

Q: Question 5, Part d: How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum…

Q: Given the half-cell reduction potentials, the overall cell reaction, and cell potential below:…

A: Dear student I have given answer to your question in the image format

Q: Reduction half-cells and their standard potentials are, respectively: N2 (g) + 4 H2O (l) + 4 e- →…

A: Answering the first three sub parts as per guidelines for further assistance please post the…

Q: 24. The following redox reaction is spontaneous as written: Ca2+(aq) + Zn(s) ⟶⟶ Zn2+ + Ca(s)…

A: Given, Chemical Reaction : Ca2+(aq) + Zn(s) ⟶⟶ Zn2+ + Ca(s)

Q: The standard reduction potentials for two pairs of redox species are shown below. These two…

A: Introduction :- A redox reaction is spontaneous if the standard electrode potential for the redox…

Q: The standard reduction voltages of F2(g) and Li*(aq) are 2.87 V and -3.04 V, respectively. What is…

A: Standard voltage of an electrochemical cell can be calculated by the following formula.…

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

A: First, let's identify the reduction and oxidation half-reactions and their potentials:- Reduction…

Q: half-reaction standard reduction potential Fe?+ (аq) .0 3+ Fe"(aq)+e E°=+0.771 V red…

A: The half reactions along with their standard reduction potential are given as, The half reaction…

Q: Consider a galvanic electrochemical cell constructed using Cr/Cr3* and Zn/Zn?+ at 25 °C. The…

A: The electrode with higher reduction potential of the metal is known as cathode. In this cathode,…

Q: 8. Calculate Eº, E, and AG for the following cell reactions: (a) Mg(s) + Sn²+ (aq) → Mg²+(aq) +…

Q: What is the concentration for Sk2+ for which s galvanic cell needs when the concentration of the…

A: for spontaneous operation of galvanic cell Ecell must be positive.

Q: 5. The following galvanic cell has a potential (E) of 0.98 V at 298 K. Zn(s) | ZnX,2* (0.010 M), X…

A: Given the potential of the cell, E = 0.98 V T = 298 K Here Zn(s) is oxidized to ZnX42+(aq) at the…

Q: Given the following half-cell reactions: Cr+3 + 3e- -> Cr E° = -0.74 V Zn+2 + 2e-…

A: Given: Cr+3+3e-→Cr Eo=-0.74 VZn+2+2e→Zn Eo =-0.83 V To determine:…

Q: Payalben

A: The objective of this question is to calculate the cell potential of an electrochemical cell at 25…

Q: The following reduction half reactions were used to create a cell: A2+ (aq) + 2 e-→ A(s)…

Q: 4. Calculate at which Zn² concentration (x) the following electrochemical cell has an EMF of 0.9 V.…

Q: Half-reaction containing acid : 3 N2 (g) + 2 H+ (aq) + 2 e- → 2 HX (aq) Eo red = -3.09 V 1. using…

A: Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: [References] If E°. cell 0.975 V for the following reaction: I2 (s) + Fe(s) → 2 I'(aq) + Fe2*(aq)…

Q: If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round…

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

Q: The free energy change for the following reaction at 25 °C, when [Ni²+] = 1.15 M and [Cd²+] =…

A: Given,

Q: For the following two reduction half-reactions, which will occur at the cathode? a) Fe3+(aq)…

A: We are given two half cell reactions as follows; Fe3+(aq) + e- ------> Fe2+(aq) Eo = +0.771…

Q: 8. Consider the cell Fe(s) FeSO.(ag) Hg.SO.(1) Hg() Write the half-cell reactions and the full cell…

A: Formulae used: E°cell = E°cathode - E°anode deltaG° = - RTlnK delta G° = -nFE°cell T = 298 K R…

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: Voltage can be calculated as follows

Q: A cell utilizes the following reaction and operates at 298 K: 2H+(aq) + Zn(s) → Zn2+(aq) + H2(g)…

A: Given that: [Zn2+] = 0.050 M P(H2) = 0.25 atm pH = 4.00 The standard cell potential is the EMF of…

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: Given reaction is : 2Ag+ (aq) + Cu (s) ------------> 2Ag (s) + Cu2+ (aq) , ΔG0 = -88660 J/mole…

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

100%

24.
Given the following half-cell reactions:
2+
Fe²+ (aq) + 2e¯¯ Fe (s)
Eº
3+
Cr³+ (aq) + 3e-
Cr (s)
a. +1.18 V
b. -0.30 V
C.
-1.18 V
Fe²+ (Aq)
1M
-0.44 V
= -0.74 V
Fe
Cr
Cp 3+
d. +0.30 V
e. +1.34 V
(Aq)
At 25°C, the initial cell voltage of the cell shown in the diagram above is
1M

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 1 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

Galvanic cell has 2 half reactions O2(g) + 4H+(aq) + 4e- → 2H2O(l) E0red = +1.23 V Cr3+(aq) + 3e- → Cr(s) E0red = -0.74 V Write a balanced equation that describes the cell, ensuring that E0cell > 0 V and Calculate E0cell
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Ni
Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous
half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V red MnO, (aq)+2 H,0(1)+3e MnO,(5)+4 OH (aq) E° =+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. 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. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If said it was you possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
3.) Consider the following standard reduction potentials, which statement is correct at standard conditions? Ni?* (aq) + 2 e → Ni (s) E°red = -0.26 V I2 (s) + 2 e -> 2 (aq) E°red = 0.54 V I. Ni²* (aq) is a stronger oxidizing agent than I2 (s), and I is a stronger reducing agent than Ni (s) II. I2 (s) is a stronger oxidizing agent than Ni2", and Ni (s) is a stronger reducing agent than I (aq) III. Ni (s) is a stronger oxidizing agent than I (aq), and Ni2* is a stronger reducing agent than I2 (s) IV. I(aq) is a stronger oxidizing agent than Ni (s), and I2 (s) is a stronger reducing agent than Ni2+ (aq) А. IV В. Ш С. П D. I
Use cell potential to calculate the standard free energy change for this reaction. MnO4- (aq) + 8 H+ (aq) + 5 Fe2+ (aq) --> MN2+ (aq) + 4 H2O (l) +5 Fe3+ (s) a. -357 kJ b. 357 kJ c. 941 kJ d. -941 kJ e. 1130 kJ
2+ 4+ a. Will Fe+ oxidize Sn to Sn*t ? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Fes+ +e → Fe2+ +0.77 Sn n4+ + 2e → Sn²+ +0.15 O yes O no b. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Cr2 0, + 14H+ + 6e¯ → 2Cr³+ + 7H2O +1.33 Cl2 + 2e → 2C1 +1.36 O yes O no
Which of the following half-reactions has been assigned a standard reduction potential, E°, of 0.00 Volts? A.) O2(g) + 4 e- → 2 O2-(aq) B.) 2 H2O(l) + 2 e- → H2(g) + 2 OH-(aq) C.) Pt + H+(aq) + e- → H-Pt D.) 2 H+(aq) + 2 e- → H2(g)
Determine E cell at 298 K when [Ni2+] = 0.33 M and [Ag+] = 0.51 M. Ni2+(aq) + 2e- -> Ni(s) Eredo =-0.257V Ag+(aq) + e- -> Ag(s) Eredo =+0.7996V
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.