Answered: At what temperature, in °C, is a…

Science

Chemistry

At what temperature, in °C, is a certain reaction at equilibrium if AH :+87.9 kJ/mol and AS = +170.2 J/ mol · K?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.20QE: The equilibrium constant for a reaction decreases as temperature increases. Explain how this...

See similar textbooks

Related questions

Q: Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → co2(g) +…

A: Given: The reaction is as follows, FeO(s) + CO(g) → CO2(g) + Fe(s) ∆H = -11.0 kJ∆S = -17.4 J/K

Q: What is the equilibrium constant for a reaction that has a ΔGrxn of -11.1 kJ at a temperature of…

A: Convert unit of temperature:

Q: Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. ΔG°f…

A: Since appendix II B is not provided, so considering the standard data: ∆G˚(NO2) = 51.3 kJ/mol…

Q: Which process would be predicted to have AS < 0? a solid melting a bond forming a solution being…

A: When atoms are more randomly or disorderly present in a substance then it is called entropy of…

Q: For a particular reaction at 231.7 °C, AG = -1357.31 kJ, and AS = 770.30 J/K. Calculate AG for this…

A: Formula: ∆Gsystem = - T∆Stotal ∆G1 = - T1 x ∆S -------(i) ∆G2 = - T2 x ∆S -------(ii)…

Q: Given the following information below, determine AGrxn at equilibrium. H2(g) + 12(g) = 2 HI(g) K, =…

A: There is the relation between the Gibbs free energy change and equilibrium const

Q: For a particular reaction at 124.1 "C, AG = -201.43 kJ, and AS = 334.55 J/K. Calculate AG for this…

Q: When solid NH4SCN is mixed with solid Ba(OH)2 in a closed container, the temperature drops and a gas…

A: Answer

Q: The value of ΔH° for the following reaction is 172.7 kJ. The value of ΔH°f for CaO(s) is __________…

A: We have given that The value of ΔH° for the following reaction is 172.7 kJ. The value of ΔH°f for…

Q: Determine the temperature of a reaction if K = 1.2 x 10 when AG° = +16.2 kJ/mol. %3D

A: The Gibbs free energy and the equilibrium constant are related by the following equation: ∆Go = -RT…

Q: For a particular reaction at 222.1 °C, AG =-848.94 kJ, and AS = 171.81 J/K. Calculate AG for this…

Q: (a) If K<<1 for a reaction, what do you know about the sign and magnitude of ΔG°? (b) If Δ…

A: a) For the reaction K<<1, the sign and magnitude of ∆G0 is predicted as shown below,

Q: Use Appendix C in your textbook to answer the following question. Consider the following reaction.…

A: The value of standard Gibbs energy change of reactants and products from appendix C - COCl2 g =-…

Q: Determine the temperature of a reaction if K = 1.2 x 10⁻⁶ when ∆G° = +12.2 kJ/mol.

Q: For the reaction, 4KClO3(s) → 3KClO4(s) + KCl(s) Calculate ΔGosys for the process at 298 K if…

A: ∆Gsyso = ∆Hsyso - T ∆Ssyso where ∆Hsyso = Standard enthalpy change of system = - 144.3 KJ x…

Q: At 869 K, ΔGo equals -82.7 kJ for the reaction, Cl2(g) 2 Cl(g). Calculate the value of ln K for…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: At 298 K, AH° is 66.4 kJ/mol and As° is 26.9 J/mol K. What is AG° for this reaction at this…

A: Given data, the temperature (T) = 298 K enthalpy changes (∆Ho) = 66.4 kJ/mol entropy changes (∆So) =…

Q: Not provided Not - 46.3 Not provided Not

A: From the given data, □G° = [Total Gibbs free energy of products] - [Total Gibbs free energy of…

Q: Calculate the temperature (in kelvins) at which the sign of AG° changes from positive to negative…

Q: Calculate Kp for the following reaction at 25°C: 2SO2(g) + O2 (g) → 2SO3 (g) For SO2(g),…

Q: [1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: A certain reaction has ∆H ° = +23.7 kJ and ∆S° = +52.4 J>K. (a) Is the reaction exothermic or…

A: ∆H ° = +23.7kJ If for any chemical reaction ∆H ° is positive, the reaction will be endothermic…

Q: For a particular reaction at 235.4 °C, AG = -307.62 kJ, and AS = 992.15 J/K. Calculate AG for this…

Q: For a certain reaction, AH° = 10 kJ and AG° = 15 kJ at 250 K. What is %3D the AS° for this reaction?…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is -63.8 kJ.…

Q: Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) CO2(8) +…

A: We have to find the Temperature for becoming a non-spontaneous reaction. Enthalpy and Entropy are…

Q: Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) and…

A: The relationship between Gibbs free energy change, enthalpy change and entropy change is given by…

Q: Calculate ΔS°, ΔSsurr and ΔSuniv 298 K for the reaction: 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

A: Given chemical reaction is shown below: 2 KClO3(s) → 2 KCl(s) + 3 O2(g) Calculate ΔS°, ΔSsurr and…

Q: Predict the sign of ∆Ssys for each of the following processes: (a) Molten gold solidifies.

A: The measurement of randomness or disorder of the system is called as entropy. It is a state function…

Q: plain briefly why the exothermic reaction of a metal carbonate with an acid is product-favored.…

A: An exothermic reaction is one that evolves heat. It is because enthalpy of products is less than…

Q: What is K for a reaction if ∆G° =173.2 kJ/mol at 25.0 °C? (R = 8.314 J/mol ･ K)

A: Given, Standard gibbs free energy (∆G°) = 173.2 kJ/mol = 173.2 × 1000 J/mol = 173200 J/mol…

Q: Determine the temperature of a reaction if K = 1.20 x 10⁻⁶ when ∆G° = +37.60 kJ/mol.

A: Formula used :- ∆G° = -2.303RTlogk ∆G° = change in Gibb's free energy k = equilibrium constant…

Q: 2NO(g) + O2(g)→ 2NO2(g); AH°= -125 kJ/mol; AS°= -150 J/mol-K Below a temperature of K, this reaction…

Q: Consider the following reaction at equilibrium. Fe3O4(s) + CO(g) = 3 FeO(s) + CO2(g) AH°= -35.9 kJ…

A: We have to tell which option is correct from given choices of options by telling effect of given…

Q: For the reaction: CCl4(g) → C(s) + 2 Cl2(g) ΔH∘∘ = +95.7 kJ and ΔS∘∘ = +142.2 J/K The…

A: The question is based on the concept of chemical thermodynamics. We have to identify the nature of…

Q: Consider the following reaction at 41°C. 2 NOCI(g) = 2 NO(g) + Cl,(9) AG° = 38.0 kJ If 1.73 atm of…

A: Given information: Temperature = 41 ℃ Gibb’s free energy change = 38.0 kJ Pressure of NOCl = 1.73…

Q: What is AG for a reaction where AG° = -4.5 kJ/mol and Q = 2.8 at 295 K? (R = 8.314 J/mol· K)

Q: For a particular reaction at 199.1 °C, AG = -159.63 kJ, and AS = 894.41 J/K. Calculate AG for this…

A: Given data for a particular reaction at temperature 199.1°C , T = 199.1°C = (199.1+ 273) K = 472.1…

Q: 4. Calculate AS in J/K for the following reaction at 25°C and 1 atm: H2SO:(aq) + 2NaOH(aq) → 2H20(1)…

A: The change in entropy can be found out by subtracting the sum of entropies of reactants to that of…

Q: Automobiles and trucks pollute the air with NO. At 2000.0°C, K, for the reaction is 6.62 x 10-4, and…

Q: Calculate AGᵒrxn in kJ for the following reaction at 550.0 K. CaCO3(s)→ CaO(s) + CO₂(g) -89040 O…

Q: Given the reactions, X(s) + 0,(g) → XO(s) AH = -527.1 kJ XCO,() - → XO(s) + CO,(g) AH = +261.3 kJ…

Q: Given the following information below, determine AGrxn at equilibrium. 12(g) + Cl2(g) 2 ICI(g) K, =…

A: Kp : This is defined as the equilibrium constant of the reaction in terms of the atmospheric…

Q: A certain reaction has ∆H ° = +23.7 kJ and ∆S° = +52.4 J>K. Calculate ∆G° for the reaction at 298…

Q: (H2 ) →(12 ) +( 2HI) (AS = 82.4 J/K ) ,(AH = 25.9 KJ/K) %3D Calculate AG for this reaction at 25 C°

A: Given, H2 ---> I2 + 2 HI ∆S = 82.4 J/K ∆H = 25.9 KJ/K ∆G = ?

Q: Use Table 6 values to calculate AG° (in kJ) at 2000 K for the following reaction: NO2 (g) + CO(g) →…

Q: A certain reaction is spontaneous at 25°C. If the enthalpy change for the reaction is 29.8 kJ/mol,…

A: Given that: T = 25°C = 25°C + 273 = 298K dHrxn = 29.8KJ/mol

Q: Calculate the value of K for the formation of NO2 from NO and O2 at 298 K if ∆?° = -35.3 kJ/ mol for…

A: Given, Standard free energy change ∆G° = -35.3 kJ/ mol R= 8.314 J/mol.K = 0.008314 KJ/mol.K T = 298…

Q: What is delta G for this reaction in kJ/mol?

A: Given :- K = 81.7 T = 25°C To calculate :- ∆G (in kJ/mol) ∆G= -RTlnk

Q: . Consider the following reaction at equilibrium: M + N Q + R AH = + 350 kJ

A: when an irreversible reaction carried out it in closed vessel , at certain time equilbium state is…

Question

100%

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 : Given

VIEW

Step 2 : Calculations

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

In the reaction 450.0⁰c: caco3(s) ⇌ cao(s) + co2(g), at equilibrium, if pco2 = 0.0160 atm , what is the value of Kc
Calculate the value of K for the formation of NO2 from NO and O2 at 298 K if ∆?° = -35.3 kJ/ mol for the following reaction. (R = 8.314 J/mol. K) NO(g) + 12 O2 (g) ⇌ NO2 (g)
For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp = 5.10×10−3 at 345 ∘C. What is Kc for the reaction at this temperature?
Calculate Kp for the following reaction: PCl3 (g) + Cl2 (g) <--> PCl2(g),Kc = 1.67 at 500
For the following reactionC(??) + 2H2(??) ⇌ CH4(??)K =0.26 at 1000 °C (3 significant figures). What is the equilibrium constant at 750 °C (3significant figures)?
At 25.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) is at equilibrium when PCO2 = 3.50 mbar, [H2O] = 55.5 mol L-1, [H+] = 39.8 µmol L-1, and [HCO3-] = 1.28 mmol L-1. Then an additional 4.00 mbar of CO2 is added to the system. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)
At 25.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) is at equilibrium when PCO2 = 3.50 mbar, [H2O] = 55.5 mol L-1, [H+] = 39.8 µmol L-1, and [HCO3-] = 1.28 mmol L-1. Then an additional 4.00 mbar of CO2 is added to the system. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1) (Hint: you will need to first perform a calculation under equilibrium conditions, and then a second calculation under non-equilibrium conditions.)
Consider the following equilibrium: 2NOBr(g) ⇄2NO(g) + Br2(g). If Kp = 4.3 × 10−3 at 300.0 K, calculate Kc.
What is K for a reaction if ∆G° =-292.8 kJ/mol at 25°C? (R = 8.314 J/mol ･ K)
What is the equilibrium pressure (in atm to three decimal places) of HBr for the following reaction if P(H2)i = P(Br2)i = 1.000 atm at 25 °C? H2(g) + Br2(g) ⇌ 2HBr(g) K=0.00550
Given the following two measurements of the equilibrium constant for a reaction, calculate ΔH° for the reaction. (kJ/mol) (no scientific notation) T, °C K 30.0 5.2 x 103 50.0 15.4 x 104
Consider a process with ∆H = -89.8 kJ and ∆S = -151 J/K. At what temperature will this process be at equilibrium?