For each of the following reactions, balance the chemical equation, calculate the emf, and calculate AG at 298 K. (Use thesmallest possible coefficients for H₂O(1), H+ (aq), and HO (aq). These may be zero.)(a) In basic solution Cr(OH)3(s) is oxidized to CrO4²- (aq) by ClO (aq).Cr(OH)3(s) +clo (aq) +OH(aq) →H₂O (1)emfAGºH₂O (1)emfAGº(b) In acidic solution copper(I) ion is oxidized to copper(II) ion by nitrate ion.Cu+ (aq) +NO3(aq) +H+ (aq) →Cu²+ (aq)VemfkJAG⁰V2+(c) Aqueous iodide ion is oxidized to I₂ (s) by Hg₂²+ (aq).H+ →I(aq) +Hg₂2+ (aq) +kJVkJCro4² (aq)1₂(s)Hg(1) +Cl(aq) +NO(g) +H₂O(l)

Answered: Image /qna-images/answer/6b3c052c-a196-4ab9-a222-97dad50c8ddc.jpg

For each of the following reactions, balance the chemical equation, calculate the emf, and calculate AG at 298 K. (Use the smallest possible coefficients for H₂O(1), H+ (aq), and HO (aq). These may be zero.) (a) In basic solution Cr(OH)3(s) is oxidized to CrO 4² (aq) by ClO (aq). Cr(OH)3(s) + clo (aq) + OH(aq) → H₂0 (1) emf AG⁰ H₂O (1) emf AGO (b) In acidic solution copper(I) ion is oxidized to copper(II) ion by nitrate ion. Cu+ (aq) + NO3(aq) + H+ (aq) - Cu²+ (aq) V emf kJ AG⁰ V (c) Aqueous iodide ion is oxidized to I₂(s) by Hg₂2+ (aq). I(aq) + Hg₂²+ (aq) + kJ V kJ H+ → Cro4² (aq) 1₂(s) Hg(/) + Cl(aq) + NO(g) + H₂O(1)

For each of the following reactions, balance the chemical equation, calculate the emf, and calculate AG at 298 K. (Use the smallest possible coefficients for H₂O(1), H+ (aq), and HO (aq). These may be zero.) (a) In basic solution Cr(OH)3(s) is oxidized to CrO 4² (aq) by ClO (aq). Cr(OH)3(s) + clo (aq) + OH(aq) → H₂0 (1) emf AG⁰ H₂O (1) emf AGO (b) In acidic solution copper(I) ion is oxidized to copper(II) ion by nitrate ion. Cu+ (aq) + NO3(aq) + H+ (aq) - Cu²+ (aq) V emf kJ AG⁰ V (c) Aqueous iodide ion is oxidized to I₂(s) by Hg₂2+ (aq). I(aq) + Hg₂²+ (aq) + kJ V kJ H+ → Cro4² (aq) 1₂(s) Hg(/) + Cl(aq) + NO(g) + H₂O(1)

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 free-energy changed) for the reaction at 25°C Use the standard reduction…

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

Q: Hydrazine has been employed as a reducing agent for metals.Using standard reduction potentials,…

A: EXPLANATION: Hydrazine is used as a reducing agent thus itself get oxidised. Reduction potential of…

Q: An iron(II) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with…

Q: Calculate the solubility product of AgCl at 25.0 °C, given the following data: AgCits)+eAg(s) +…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Given-> [Cr2+] = 0.790 M [Fe2+] = 0.0190 M T = 25°C

Q: In a galvanic cell, one half-cell consists of a tin strip dipped into a 1.00 M solution of Sn(NO3)2.…

A: Given , Cell voltage = 0.595 V

Q: Write the balanced half-reaction corresponding to the oxidation involved in the air oxidation of…

A: Answer: During the rusting of Iron a galvanic cell forms on its surface and a redox reaction takes…

Q: Calculate the cell potential for the reaction as written at 25.00 °C25.00 °C, given that…

A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.768 M [Fe+2] = 0.0170 M

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: Determine the equilibrium constant, Keq, at 25oC for the reaction: Au3+(aq) + Li(s) → Au(s) +…

A: The reaction given is Au3+(aq) + Li(s) → Au(s) + Li+(aq)

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) Ti² (aq) +…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

Q: Calculate the change in standard Gibbs energy (AC), in kilojoules, for the reaction below at 25 °C.…

Q: Predict whether the following reaction would proceed spontaneously as written at 298 K:…

A: Co(s) + Fe2+(aq) -> Co2+(aq) + Fe(s)[Co2+] = 0.15M and [Fe2+] = 0.68MReduction potential values,…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…

Q: Calculate the cell potential for the galvanic cell in which the reaction Cd(s)+Cu2+(aq)↽−−⇀…

Q: (a) Liquid H2O is subjected to electrolysis. One of the half-reactions is 2 H2O → O2 (g) + 4 H+(aq)…

A: We have to calculate the Faraday of electricity required and the time taken.

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: Four metals, A, B, C, and D, exhibit the following properties. (a) Only A and C react with l.0 M…

A: The reducing agent is defined as the species( elements, compounds, metals) which tend to give away…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M

Q: The following reactions are all observed to occur spontaneously as written. Ti(s) + Pd2+ (aq) → Ti²+…

A: All the given reactions are redox reactions. One of the reactants gets oxidized (oxidation state is…

Q: Calculate the equilibrium constant for the following reaction at 25 °C, Co(s) +2 Cr3+ (aq) → Co2+…

Q: can cadmium metal (Cd(s)) reduce cobalt (II) ions (Co2+(aq)) to cobalt metal

A: cadmium can only reduce cobalt if its reduction potential is smaller than that of cobalt.

Q: An aqueous solution of an unknown salt of molybdenum is electrolyzed by a current of 2.50 A passing…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.807 M and…

Q: Which of the following reactions has the largest equilibrium constant (K) at Standard Conditions?…

A: Keq = [Product]/[Reactant] However, the concentration of liquid and solid is taken as 1.

Q: A current of 13.4A is passed through an electrolysis cell containing molten NaCl for 16.8 minutes.…

A: The objective of the question is to predict the products of electrolysis of molten NaCl and to…

Q: Calculate the standard free-energy change, in kilojoules, at 25 °C for the reaction 2 Ag* (aq) + Zn…

Q: Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe*(aq) + B(s) + 6H,O(1) -…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M…

A: Given data : Cr(s) + Fe2+ (aq) ==> Cr2+(aq) + Fe(s) From table : E(Fe2+/Fe) = -0.44 V…

Q: What is the balanced chemical equation for this galvanic cell reaction? Cr(s) | Cr3*(aq), 1M || CI-…

Question

100%

For each of the following reactions, balance the chemical equation, calculate the emf, and calculate AG at 298 K. (Use the
smallest possible coefficients for H₂O(1), H+ (aq), and HO (aq). These may be zero.)
(a) In basic solution Cr(OH)3(s) is oxidized to CrO4²- (aq) by ClO (aq).
Cr(OH)3(s) +
clo (aq) +
OH(aq) →
H₂O (1)
emf
AGº
H₂O (1)
emf
AGº
(b) In acidic solution copper(I) ion is oxidized to copper(II) ion by nitrate ion.
Cu+ (aq) +
NO3(aq) +
H+ (aq) →
Cu²+ (aq)
V
emf
kJ
AG⁰
V
2+
(c) Aqueous iodide ion is oxidized to I₂ (s) by Hg₂²+ (aq).
H+ →
I(aq) +
Hg₂2+ (aq) +
kJ
V
kJ
Cro4² (aq)
1₂(s)
Hg(1) +
Cl(aq) +
NO(g) +
H₂O(l)

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 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

(a) A student is required to construct a battery in the form of a galvanic cell using nickel (II) nitrate and cadmium (II) nitrate. Given that a 0.75 M solution of nickel (II) nitrate must be used, what concentration of cadmium nitrate is required to achieve a cell voltage of 0.12 V at 25 °C? Ni*(aq) + 2e° → Ni(s) Cd²*(aq) + 2e → Cd(s) E°red= - 0.40 V E°red = - 0.26 V 2.
Determine the equilibrium constant at 25 ºC for the dissolution of magnesium hydroxide in acidic solution: Mg(OH)2 (s) + 2H + (aq) ⇌ Mg 2+ (aq) + 2H2O (l)
Copper(I) ion can act as both and oxidizing agent and a reducing agent. Hence, it can react with itself. Using the data provided below, calculate the equilibrium constant, K, for the following reaction at 25 °C from standard electrode potentials. 2Cu+(aq) ----> Cu(s) + Cu2+(aq) Express your answer to three significant figures. Cu2+(aq) + e- ----> Cu+(aq) E° = 0.16 V Cu+(aq) + e- ----> Cu(s) E° = 0.52 V Note: Your answer is assumed to be reduced to the highest power possible.
With the information provided below, calculate the enthalpy of reduction, AredHº, for the reaction: Sr2*(aq) → Sr(s), and comment on the sign of the obtained magnitude given the properties of the alkaline-earth elements (i.e.: metallic character, reduction potentials, etc.). (hint: Hess' law should come in handy) Show your work AatH® (kJ/mol) AnyaH® (kJ/mol) IE: (kJ/mol) IE2 (kJ/mol) Element Sr 164 -1456 549.5 1064 AatHº: enthalpy of atomization; AnyaH®: enthalpy of hydration; IE1: first ionization energy; IE2: second ionization energy 2.
Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the cathode. Calculate the time it takes to deposit 0.34 gram of gold, passing a current of 0.10 amperes. (1 faraday = 96,485 coulombs)
7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s) + 2e → Cd (s) + 2 OH (aq) Eºred = -0.76 V NIO(OH) (s) + H₂O (1) + e → Ni(OH)2 (aq) + OH (aq) Eºred = +0.49 V Calculate the standard emf of the nickel-cadmium (nicad) rechargeable battery. *hint: the reaction for the discharge of nicad battery is: Cd (s) + 2 NIO(OH) (s) + 2 H₂O (1)→ 2Ni(OH)2 (aq) + Cd(OH)2 (s) (b) A typical nicad voltaic cell generates an emf of +1.30 V. Why is there a difference between this value and the one you calculated in part (b)? (c) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.
Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.
19. (a) Write a balanced equation for the reaction that occurs in a car battery when the ignition key is turned on. (b) Suppose that constant current of 450 A flowing through the engine for at least 10.0 seconds is needed to start a pick-up truck. How many grams of lead are consumed during this time? (c) If the battery operates at 12 V of potential, how much energy (in kJ) is produced?
Consider the following reaction at 298K.2 Cu2+ (aq) + Co (s) 2 Cu+ (aq) + Co2+ (aq)Which of the following statements are correct?Choose all that apply. K < 1 n = 4 mol electrons The reaction is product-favored. Eocell > 0 delta Go > 0
Complete and balance the following equations for reac- tions taking place in acidic solution. (a) MnO, (aq) + H,S(aq) → Mn²+ (aq) + SO? (aq) (b) Zn(s) + NO, (aq) → Zn²* (aq)+ NH (aq) (c) H,O,(aq)+ MnO, (aq) (d) Sn(s) + NO3 (aq) (e) UO* (aq) + Te(s) → U** (aq) + TeOž¯ (aq) → 02(g) + Mn²* (aq) 4+ → Sn** (aq) + N2O(g)
A tin(II) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with itself. 10 2Sn+ (ag) Sn() + Sn (ag) Calculate the equilibrium constant at 25°C for this reaction. You may need to use the following data: Standard Cathode (Reduction) Half-Reaction Potential, E (V) Sn (ag) + 2e Sn+ (aq) 0.15 Sn+ (ag)+2e Sn(s) -0.14
What is the balanced reaction for the following galvanic cell?Cr(s)| Cr3+(aq) || Fe3+(aq) | Fe(s) Fe(s) + Cr(s) ↔ Fe3+(aq) + Cr3+(aq) Fe3+(aq) + Cr3+(aq) ↔ Fe(s) + Cr(s) Fe3+(aq) + Cr(s) ↔ Fe(s) + Cr3+(aq) Fe(s) + Cr3+(aq) ↔ Fe3+(aq) + Cr(s)