Soft matter and interfacial chemistry: (c) The nitrate radical NO3 is a naturally occurring nitrogen oxygen species that accumulates inthe atmosphere at night. The steady state concentration of NO3 depends not only on itsformation and loss, but also on its conversion to and reformation from N₂O5.NO₂+O3 → NO3 + O₂N₂O5 + MN₂O5 + X→ productsNO₂ + NO3 + MK₁K₂/K-2K3(i) Explain the role of the species M in step 2 and comment on the reaction conditions thattypically require its presence.(ii) Provide an explanation on why the concentration of NO3 increases at night, your answershould include a possible reaction.

The above reaction is a three-step reaction, in which one of the steps is a reversible one.

(c) The nitrate radical NO3 is a naturally occurring nitrogen oxygen species that accumulates in the atmosphere at night. The steady state concentration of NO3 depends not only on its formation and loss, but also on its conversion to and reformation from N₂O5. NO₂ + 03 → NO₂ + NO3 + M = N₂O5 + X→ NO3 + O₂ N₂O5 + M products K₁ K₂1k-2 K3 (i) Explain the role of the species M in step 2 and comment on the reaction conditions that typically require its presence. (ii) Provide an explanation on why the concentration of NO3 increases at night, your answer should include a possible reaction.

(c) The nitrate radical NO3 is a naturally occurring nitrogen oxygen species that accumulates in the atmosphere at night. The steady state concentration of NO3 depends not only on its formation and loss, but also on its conversion to and reformation from N₂O5. NO₂ + 03 → NO₂ + NO3 + M = N₂O5 + X→ NO3 + O₂ N₂O5 + M products K₁ K₂1k-2 K3 (i) Explain the role of the species M in step 2 and comment on the reaction conditions that typically require its presence. (ii) Provide an explanation on why the concentration of NO3 increases at night, your answer should include a possible reaction.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 92QRT

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Adenosine triphosphate, ATP, is used as a free-energy source by biological cells. (See the essay on page 624.) ATP hydrolyzes in the presence of enzymes to give ADP: ATP(aq)+H2O(l)ADP(aq)+H2PO4(aq);G=30.5kJ/molat25C Consider a hypothetical biochemical reaction of molecule A to give molecule B: A(aq)B(aq);G=+15.0kJ/molat25C Calculate the ratio [B]/[A] at 25C at equilibrium. Now consider this reaction coupled to the reaction for the hydrolysis of ATP: A(aq)+ATP(aq)+H2O(l)B(aq)+ADP(aq)+H2PO4(aq) If a cell maintains a high ratio of ATP to ADP and H2PO4 by continuously making ATP, the conversion of A to B can be made highly spontaneous. A characteristic value of this ratio is [ATP][ADP][H2PO4]=500 Calculate the ratio [B][A] in this case and compare it with the uncoupled reaction. Compared with the uncoupled reaction, how much larger is this ratio when coupled to the hydrolysis of ATP?
Consider the reaction 2SO2(g)+O2(g)2SO3(g) (a) Calculate G at 25C. (b) If the partial pressures of SO2 and SO3 are kept at 0.400 atm, what partial pressure should O2 have so that the reaction just becomes nonspontaneous (i.e., G=+1.0 k J)?
Cobalt(II) chloride hexahydrate, CoCl26H2O, is a bright pink compound, but in the presence of very dry air it loses water vapor to the air to produce the light blue anhydrous salt CoCl2. Calculate the standard free-energy change for the reaction at 25C: CoCl26H2O(s)CoCl2(s)+6H2O(g) Here are some thermodynamic data at 25C: What is the partial pressure of water vapor in equilibrium with the anhydrous salt and the hexahydrate at 25C? (Give the value in mmHg.) What is the relative humidity of air that has this partial pressure of water? The relative humidity of a sample of air is Relativehumidity=partialpressureofH2O(g)inairvaporpressureofwater100 What do you expect to happen to the equilibrium partial pressure over the hexahydrate as the temperature is raised? Explain.
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.
What is a nonspontaneous reaction?
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?
7-69 Pure carbon exists is several forms, two of which are diamond and graphite. The conversion of the diamond form to the graphite form is exothermic to a very slight extent. How is it that jewelers can advertise "Diamonds are forever"?
Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.
a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?
For the following reactions at constant pressure, choose the correct relationship between AH and AE. 2HF(g) → H2(g) + F2(g) ΔΗ>ΔΕ ΔΗ ΔΕ Ο ΔΗ ΔΕ ΔΗ<ΔΕ ΔΗ-ΔΕ depends on the conditions
6. For a chemical reaction of: 3A + B 2C at 310 K for the initial conditions of: [A] = 25 mM, [B] = 52 mM, [C] = 13 mM with %3D H = 7.27 kJ/mole, u, =8.34 kJ/mole, 4 = 0.56 kJ/mole Calculate the value of AG for this process. Calculate the value of AG for this process. (A) (B) (C) Calculate K, for this process. (D) Will this reaction spontaneously proceed in the forward or reverse direction? Why?

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