Calculate Ecel for the reaction under the following nonstandard conditions and decide whether the reaction will occur spontaneously: pH 10, PO2PO2= 0.20 atm, [MNO.] = 1.0 × 10* M, and T = 25°C. 4MNO:(s) + 30:(9) + 40H-(aq) → 4MNO, (aq) + 2H:0(1) E° = -0.20 V

Calculate Ecel for the reaction under the following nonstandard conditions and decide whether the reaction will occur spontaneously: pH 10, PO2PO2= 0.20 atm, [MNO.] = 1.0 × 10* M, and T = 25°C. 4MNO:(s) + 30:(9) + 40H-(aq) → 4MNO, (aq) + 2H:0(1) E° = -0.20 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: Consider the following half-reactions: Half-reaction E° (V) 2+, Hg"(aq) + 2e¨ → Hg(1) |0.855V "(аq)…

A: Solving only first three subparts in accordance with the guidelines. We will use standard reduction…

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given, Current = 62.7 A Time = 81.9 min NaNO2 (aq) + H2O (l) NO (g) + O2 (g) + NaOH (aq)…

Q: 14.55 Complete and balance the following oxidation-reduction reactions, assuming they occur in…

A: Oxidation is the loss of electrons and increase in oxidation number takes place while the reduction…

Q: What is the equilibrium constant of the following reaction at 25°C? BrO-(aq) + H₂O(l) ≥ HBrO(aq) +…

Q: Calculate the value of AGn for the following reaction at 280 K. Ką= 2.9 × 10-8 and assume Ka does…

A: Given K = 2.9 × 10-8 T = 280°K

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

Q: calculate the equilibrium constant for each of the reactions below Pb2+(aq)+Mg(s)→Pb(s)+Mg2+(aq)…

Q: Calculate ΔGo based on the equation from the following line notation. IO4-1(aq) + 2H+1(aq) + 2e-1…

A: Given data: Eo of IO4- half-cell = 1.60 V Formula used:

Q: Complete and balance the following oxidation-reduction reactions, assuming they occur in basic…

Q: Given the data below, calculate E°cell for the reaction below. 3Cu(s) + 2NO3-(aq) + 8H+(aq) ---->…

Q: Given the information below. Is the cell spontaneous in the forward or reverse directions? Pt |…

A: Given that, Pt | Pt2+|| Au3+| Au Pt2+(aq) + 2 e– ----> Pt(s) ; E° = 1.20 Au3+(aq) + 3 e–…

Q: The reaction between iodide ion, I, and I, to form triiodide ion, I;", is shown below. Calculate AG°…

A: Kc is the equilibrium constant at concentration C. ∆Go is the standard Gibbs free energy. Data…

Q: A galvanic cell is powered by the following redox reaction: 5 Cl,(9) + I,(s) + 6 H,O(1) - 10 Cl (aq)…

A: At cathode reduction takes place while oxidation takes place at anode in galvanic cell.

Q: In an electrochemistry experiment a student used an unknown metal that was known to undergo this…

A: Given: Mass of M reacted = 0.600 g And moles of H2 produced = 5.44 × 10-3 mol.

Q: The standard free energy change at 25.00°C for the dissociation of 0.1546 M hydrofluoric (a weak…

A: Answer:- This question is answered by using the simple concept of calculation of ionisation constant…

Q: 15. What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe2+(aq)…

Q: Consider the following half-reactions: Half-reaction E° (V) 2(s) + 2e 21°(aq) 0.535V Ni2+ "(aq) +…

A: We are given the standard reduction potentials of different half cell reactions. We must know that…

Q: Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F°(aq) 2.870V 2+ Pb"(aq) +…

Q: 2C1 (aq)+2HNO, (aq)+ 2H" (aq) Cl, (g) + 2NO (g) +2H,0 (1) Data Br2(1)+2e-2Br (aq) Ca2+(aq)+2e+Ca(s)…

A: Given-> 2Cl-(aq) + 2HNO2 (aq) + 2H+(aq) ---> Cl2(g) + 2NO(g) + 2H2O(l)

Q: What is the relationship between E° and the equilibrium constant, K?

A: Standard electrode potentialE∘ is the measure of tendency of metallic electrode to loss/gain…

Q: What is the standard free energy (in kJ/mol) and the value of the equilibrium constant, K, for the…

Q: Use the References to access important values if needed for this question. Consider the following…

A: Oxidizing agent - It is the substance which gets reduced easily and oxidizes others Reducing agent…

Q: Table 20.2 Half-reaction Ee (V) Cr3+ (aq) + 3e- - Cr (s) -0.74 Fe2+ (aq) + 2e- - Fe (s) -0.440 Fe3+…

A: The given reaction is reduction half cell and for all reactions, the reduction potential is given.…

Q: alculate the value of E°cell and AG° for the following reaction as it is writter Au(s) + Ca2*(aq) -…

A: The solution is as follows:

Question

Calculate Ecel for the reaction under the following nonstandard conditions and decide whether the
reaction will occur spontaneously: pH 10, PO2PO2= 0.20 atm, [MNO.] = 1.0 × 10* M, and T =
25°C.
4MNO:(s) + 30:(9) + 40H-(aq) → 4MNO.(aq) + 2H;O(1)
E°c = -0.20 V

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

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 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

9. Write a Nernst expression, at 25 °C, for the following half-reactions: (a) Zn* (aq) + 2 e- 5 Zn (s) (b) Fe* (aq) + e- s Fe2* (aq) (c) 2 H* (aq) + 2 e- H2 (g) (d) Cr2O2- (aq) + 6 e + 14 H* (aq) S 2 Cr* (aq) + 7 H2O (I)
Give the standard line notation for each cell. (a) 2 IO3(aq) + 10 Fe²+ (aq) + 10 H+ (aq) 10 Fe³+ (aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Fe³+ (aq), I₂ (aq) || Fe²+ (aq), IO3¯(aq), H+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), Fe³+ (aq) || IO3(aq), H+ (aq), I₂ (aq) | Pt(s) Pt(s) | IO3(aq), H+ (aq), I₂ (aq) || Fe²+ (aq), Fe³+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), IO3¯¯(aq), H+ (aq) || Fe³+ (aq), I₂ (aq) | Pt(s) (b) (c) (d) Zn(s) + 2 Ag+ (aq) = Zn²+ (aq) + 2 Ag(s) Ag(s) | Zn²+ (aq) || Ag+ (aq) | Zn(s) Zn(s) | Zn²+ (aq) || Ag+ (aq) | Ag(s) Ag(s) | Ag+ (aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag+ (aq) || Zn²+ (aq) | Ag(s) H₂O₂ (aq) + 2 H+ (aq) + 2e → 2 H₂O(l) O2(g) + 2 H+ (aq) + 2 e¯ → H₂O₂ (aq) Pt(s) | H₂O₂ (aq) | Pt(s) ○ Pt(s) | O₂(g) | H₂O₂ (aq), H+ (aq) || H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq), H+ (aq) || O₂(g) | H₂O₂ (aq), H+ (aq) | Pt(s) ○ Pt(s) | H₂O₂ (aq) | O₂(g) || H+ (aq) | Pt(s) Mn²+ (aq) + 2 e → Mn(s) Fe³+ (aq) + 3e → Fe(s) Fe(s) | Mn²+ (aq) || Fe³+ (aq) | Mn(s) Mn(s) | Mn²+ (aq) || Fe³+ (aq) | Fe(s)…
(a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 91.2 A for a period of 60.1 min? The unbalanced chemical reaction representing this electrolysis is shown below.NaCl(aq) + H2O(l) Cl2(g) + H2(g) + NaOH(aq)__________ liters of Cl2(g) is generated by this electrolysis.(b) How many moles of NaOH(aq) are formed in the solution in this process? _______moles of NaOH(aq) are formed.
Consider the following acidic reaction at constant temperature: HCIO2 (aq) H+ (aq) + CIO2 (aq), Ka = 0.011 Calculate [HCIO2leq if [HCIO2]0 = 0.072 M.
Give the standard line notation for each cell. (a) 2 IO3¯(aq) + 10 Cr²+ (aq) + 10 H+ (aq) ⇒ 10 Cr³+(aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Cr²+ (aq), IO3¯(aq), H+ (aq) || Cr³+ (aq), I2 (aq) | Pt(s) Pt(s) | Cr³+ (aq), I2 (aq) || Cr²+ (aq), 103¯(aq), H+ (aq) | Pt(s) Pt(s) | IO3¯(aq), H+ (aq), I2 (aq) || Cr²+ (aq), Cr³+ (aq) | Pt(s) Pt(s) | Cr²+ (aq), Cr³+ (aq) || IO3¯¯(aq), H† (aq), I₂ (aq) | Pt(s) (b) (c) (d) Co(s) + 2 Ag+ (aq) ⇒ Co²+ (aq) + 2 Ag(s) Co(s) | Ag+ (aq) || Co²+ (aq) | Ag(s) (aq) || Ag* (aq) | Co(s) Ag(s) | Co²+ 2+ Ag(s) | Ag+ (aq) || Co²+ (aq) | Co(s) 2+ Co(s) | Co²+ (aq) || Ag+ (aq) | Ag(s) H2O2(aq)+2 H*(aq)+2e O₂(g) + 2 H+(aq) + 2 e¯ → H2O2(aq) Pt(s) | H₂O₂ (aq) | 02 (9) || H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq) | Pt(s) Pt(s) | H₂O2 (aq), H+ (aq) || O2(g) | H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | O2(g) | H₂O2 (aq), H† (aq) || H₂O2 (aq), H† (aq) | Pt(s) 00 Mn²+ (aq) + 2 e → Mn(s) → 2H,O(l) 3+ Fe³+ (aq) + 3 e → Fe(s) Eº E° -1.18 V 3+ Fe(s) | Fe³+ (aq) || Mn²+ (aq) | Mn(s) Fe(s) | Mn²+ (aq)…
For the following redox reaction calculate the Ecell and K at 298 K. 2Na+(aq) + Ca(s)→2Na(s) + Ca2+(aq) Half Reaction E(V) Na+(aq) + e- → Na(s) -2.71 Ca2+(aq) + 2e- → Ca(s) -2.87
The equilibrium constant for the reaction, HBrO(aq) + H2O ⇌ H3O+(aq) + BrO-(aq) is 2x10-9. Determine the concentration of H3O+ in a 0.05M solution of hypobromous acid.
| Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- -Cr(s) Fe2+ (aq) -0.74 + 2e- -Fe (s) -0.440 Fe3+ (aq) + e- - Fe2+ (s) Snt+ (aq) +0.771 + 2e- - Sn2+ (aq) +0.154 Which of the following reactions will occur spontaneously as written? 2Cr (s) + 3FE2+ Sn4+ (ag) + Fe2+ 3FE2+ (ag) + Cr3+ (aq) → Cr (s) + 2Cr3+ (ag) + 3Sn2+ (aq) → 3Sn4+ (aq) + 2Cr (s) (s) → 3Fe (s) + 2Cr3+ (aq) (s) → Sn2+ (aq) + Fe (s) 3FE3+ (aq)