Photochemical smog is formed through a sequence of reactions, the4.fırst of which is N2(g) + O2(g)→2NO(g). A H° for this reaction is180.6 kJ/mol. Determine the minimum temperature at which thisreaction becomes spontaneous. Assume that A H° and A Sº do notvary with temperature.SubstanceS° (J/mol*K)N2(g)191.5O2{g)205.0NO(g)210.6NO2(g)240.5O(g)161.0This reaction will not be spontaneous at any temperature.7039 oC7585 oCThis reaction is spontaneous at all temperatures.7312 oC

Answered: Image /qna-images/answer/99b51736-1194-46e9-a3c6-a46c7667f7c9.jpg

Photochemical smog is formed through a sequence of reactions, the fırst of which is N2(g) + O2(g) –→ 2NO(g). A H° for this reaction is 180.6 kJ/mol. Determine the minimum temperature at which this reaction becomes spontaneous. Assume that A Hº and A Sº do not vary with temperature.

Photochemical smog is formed through a sequence of reactions, the fırst of which is N2(g) + O2(g) –→ 2NO(g). A H° for this reaction is 180.6 kJ/mol. Determine the minimum temperature at which this reaction becomes spontaneous. Assume that A Hº and A Sº do not vary with temperature.

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: A chemical reaction has a standard entropy change, ΔSo, of -287.8 J/(molK) and a standard enthalpy…

A: The given data you have - ΔSo = -287.8 J/K-mol ΔHo = -138.1 kJ/mol

Q: Below what temperature does the following reaction become spontaneous? FeO(s) + CO(g) → CO2(g) +…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: 1. chemical reactions between liquids can produce gaseous products. For instance, in an…

Q: Photochemical smog is formed through a sequence of reactions, the first of which is N2(g) + O2(g) ⟶…

A: For a reaction to be spontaneous , should be negative Hence value of should be greater than ,

Q: Consider the process of water boiling in a beaker that is open to the atmosphere. Which of the…

A: In the given question, we are boiling water in a beaker and then have to see its thermodynamic…

Q: For a particular chemical reaction DH = 6.8 kJ and DS = –29 J/K. Under what temperature condition is…

A: Gibbs Helmholtz Equation: Is the equation denoted by,…

Q: Consider this reaction: N2 (s) + 2 02 (g)→ 2NO2 (g) AS° = -121.77 J/K.mol; AH° = %3! 66.36 kJ/mol…

A: From the given question it is given that, ΔSo < 0 ΔH0 > 0

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: Answer:A chemical reaction can only be spontaneous when is less than zero and value of is:Here: T…

Q: Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) +3 02(g) - 2…

A: Given, The balanced chemical equation is given below, 2H2O(g)+3O2(g)→2SO2(g)+2H2O(g) Then, ∆H=-1036…

Q: Given the following table of thermodynamic data, Substance ΔH∘f(kJ/mol) S∘(J/mol⋅K) H2(g)…

A: The "spontaneous reactions" always favor "forward reactions" where more product gets yielded and…

Q: Identify whether the following process is spontaneous or nonspontaneous. Explain your answer.…

A: Given process, Dissolving table salt in boiling water. Melting ice at 25.0°C.

Q: 17. For the reaction: A + B → C AH°= +300 kJ/mol and AS° = +200 J/K.mol. At what temperature will…

A: Given, ∆H° = 300kJ/mol ∆S° = 200J/K.mol

Q: AH°rxn = -150 kJ/mol and AS°rxn = -413 J/mol* АВ (g) + 2C (g) > АВС2 (g) plied reaction data, what…

A: A reaction is spontaneous when value of change in Gibbs Free Energy is negative i.e. value of ∆G.

Q: Consider the following reaction at constant pressure. Use the information below to determine the…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: A reaction is said to be spontaneous if a change in Gibbs free energy is negative.…

Q: The sun catalyzes the atmospheric reaction as seen below. 2N2O(g)+O2(g)→4NO(g) This reaction would…

A: Answer :- The reaction will have a Positive ΔS , because the moles of gas increases.…

Q: What is the entropy change when 2.50 moles of CCl₂F₂ vaporizes at 25.0 °C? [∆H(vap) = 17.2 kJ/mol at…

A: Given data is Moles of CCl2F2 vaporized = 2.50 ∆H(vap) = 17.2 kJ/mol at 25.0 °C

Q: The graph below shows the change in Gibbs free energy for two reactions. Change in Gibbs Free Energy…

A: According to Thermodynamics, ∆G>0 = non spontaneous ∆G< 0 = spontaneous ∆G = 0 , At…

Q: 1: Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → →…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

Q: Calculate q, AH and AU for the process during which 2 mol NO2 is heated at a constant pressure of 1…

Q: The standard enthalpy change and standard entropy change for the reaction are: A,HP = -666.2 kJ…

A: The spontaneous nature of the reaction is determined by calculating the change of free energy of the…

Q: For a reaction in which ∆H = 76.2 kJ/mol and ∆S = 422 J/K mol, determine the temperature, in °C,…

A: We have the equation for Gibbs free energy as, ∆G = ∆H-T∆S Where, ∆G = change in Gibbs energy ∆H =…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: Given physical or chemical change:A gas expands, absorbing heat from the surroundingsDuring an…

Q: Example: What is the temperature range in which the following reaction is spontaneous? N₂+ 3H2 →…

A: The change in entropy (ΔS) for a reaction can be calculated using the formula:ΔS=ΣS−ΣSwhere ΣS is…

Q: Which statement is true for the temperature dependence of the reaction below if DH = 1319 kJ/mol and…

Q: Classify each of the following reactions as spontaneous only at low temperatures (i), only at high…

Q: For the process O2(g) 2O(g), ΔH° = 498 kJ·mol –1. What would be the predicted sign of ΔS°rxn…

A: Given that :Reaction = O2(g) → 2O(g) ∆H° = 498kJ/mol

Q: Cl₂ is a stable diatomic molecule. It can be decomposed to form two Cl atoms as shown here: Cl₂(g) →…

A: Answer:Here:

Q: Which reaction is spontaneous only at a lower temperature? O 2H₂SO (1) 2SO₂(g) + 2H₂O(g) + O₂(g)…

A: If ΔG > O means reaction is non-spontaneousIf ΔG< O means reaction is spontaneousIf ΔG = O…

Q: Example: What is the temperature range in which the following reaction is spontaneous?N2 + 3H2 →…

A: Step 1:Step 2:

Q: 64. For each reaction, calculate AHxn, ASixn, and AGxn at 25 °C and state whether or not the…

A: To solve this problem, we will first need to find the standard enthalpy change (H°rxn), standard…

Q: What is the entropy change when 2.30 moles of CCl₂F₂ vaporizes at 25.0 °C? [∆H(vap) = 17.2 kJ/mol at…

A: Answer: Entropy is the measure of randomness of the system. In more possible states system can…

Q: SUBSTANCE ENTHALPY ENTROPY Ca3(G) 112 KJ mol 153.37 J/mol K CI7(G) 203.12 KJ mol 213.80 J/mol K…

Q: о Example: What is the temperature range in which the following reaction is spontaneous? N₂+ 3H2 →…

A: The problem is asking for the temperature range in which the reaction of nitrogen and hydrogen to…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: Spontaneity of the reaction can be decided on the basis of the value of Gibbs free energy change…

Q: Determine the amount of free energy of the reaction at 25 ℃ represented by the equation below. Is…

A: ∆G° = ∆H° - T∆S° So in this reaction first determine ∆H° and ∆S° then determine ∆G° If ∆G° < 0…

Q: Determine AGº for the reaction 2 NO₂(g) → 2 NO(g) + O₂(g) at 25 °C. Substance NO₂ (g) NO (g) AG°f…

A: The standard Gibbs free energy change of the reaction is calculated as follows:

Q: Which of the following statements accurately describes the spontaneity of the reaction below?…

Q: Which statement is true of the internal energy of the system and its surroundings following a…

A: The first law of thermodynamics states that the energy of the universe is constant i.e. the sum of…

Q: A,H° -1115 kJ/mol = PC13(/) + 1.5 H₂(g) → PH3(g) + 1.5 Cl₂(g) A,H° = +325 kJ/mol H₂O(g) + 0.5 O₂(g)…

Q: The enthalpy for a certain process is 146.4 kJ/mol and the entropy for the process is 463.6 J/K. At…

Q: Above what temperature does the following reaction become non-spontaneous? 2 H₂S(g) + 3 O₂(g) → 2…

A: For a reaction to be spontaneous,its delta G must be negative.So let us try to calculate a…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: In chemistry, a spontaneous process is one that occurs naturally under certain conditions without…

Question

Photochemical smog is formed through a sequence of reactions, the
4.
fırst of which is N2(g) + O2(g)→
2NO(g). A H° for this reaction is
180.6 kJ/mol. Determine the minimum temperature at which this
reaction becomes spontaneous. Assume that A H° and A Sº do not
vary with temperature.
Substance
S° (J/mol*K)
N2(g)
191.5
O2{g)
205.0
NO(g)
210.6
NO2(g)
240.5
O(g)
161.0
This reaction will not be spontaneous at any temperature.
7039 oC
7585 oC
This reaction is spontaneous at all temperatures.
7312 oC

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 with 2 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

For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
From the values of ΔH and ΔS calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -389 kJ/mol, ΔS = 27.8 J/K · mol
For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g) , ∆Horxn = -236.0 kJ
Howwwwww
For the reaction 2 A(g) → A2(g), Q = -20.00 kJ for the formation of onemole of A2(g) at constant volume and a temperature of 25.00◦C. If we did thissame reaction at constant pressure, what would be the values of Q, W, ∆U,and ∆H for the formation of one mole of A2(g) at a temperature of 25.00◦C?
Nitric oxides, NONO and NO2NO2, contribute to air pollution, acid rain, and the depletion of the ozone layer. After NONO forms in the combustion chamber of an automobile engine, it reacts further with oxygen to form NO2NO2. The reaction is given by: 2NO(g)+O2(g)→2NO2(g). Calculate ΔS∘rxn for the reaction? Entropy values given by following table SubstanceSubstance S∘ (J/mol⋅K)S∘ (J/mol⋅K) NO2NO2 240.0 O2O2 205.2 NONO 210.8
Consider the reaction below for the decomposition of carbon tetrachloride gas: CCl4(g) ------> C(s) + 2Cl2 (g) ΔH = + 95.7 kJ; ΔS = + 142.2 J/K If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.
From the values of ΔH and ΔS predict which of the following reactions would be spontaneous at 25°C. Calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -75.8 kJ/mol, ΔS = 126 J/K · mol
The enthalpy and entropy changes for a reaction at 298 K are ∆H = 46 kJ and ∆S = 190 J/K. Which of the following best describes this reaction A) The reaction is spontaneous and driven by favorable changes in the enthalpy and entropy. B) The reaction is not spontaneous because heat is absorbed. C) The reaction is not spontaneoius but could be spontaneous at a higher temperature. D) The reaction is spontaneous and driven by the favorable entropy change.
Which are spontaneous at all temperatures? Choose one or more: 2H,0(g) + SO,(g) - 152.4 J/K 2H,S(g) +30,(g) AH°. rxn = - 1037 kJ, AS°. rxn → 2SO3(g) - 197.8 kJ, ASº. 2SO,(g) +O2(g) AH°. rxn - 187.8 J/K rxn O so,(8) + H,0(1) → H,SO4(1) AH°. rxn - 132.5 kJ, AS° - 169.9 J/K rxn S(g) +O2(8) –→ SO,(g) - 574.0 kJ, AS°, ΔΗ. rxn - 124.6 J/K rxn none of the above