The standard state Gibb's energy and entropy changes are known for the reaction: 2H,S(g) + 30,(g) =2H20(g) + 2SO2(g) What is the standard state enthalpy change for the reaction at 25 C? 120 kJ 52 J AGº AS Mole Mole K -68 kJ/mol 154 kJ/mol 104 kJ/mol -119 kJ/mol

The standard state Gibb's energy and entropy changes are known for the reaction: 2H,S(g) + 30,(g) =2H20(g) + 2SO2(g) What is the standard state enthalpy change for the reaction at 25 C? 120 kJ 52 J AGº AS Mole Mole K -68 kJ/mol 154 kJ/mol 104 kJ/mol -119 kJ/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 93QRT: The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar...

See similar textbooks

Related questions

Q: 50. For the process O2(g) → 2 O(g), AH° = +498 kJ. What would be predicted for the sign of ASrxn and…

A: 50. The given process has a positive sign for enthalpy change. Hence, the process will be an…

Q: Do exothermic or endothermic reactions have a greater tendency to be spontaneous, and why? IUse the…

A: A spontaneous reaction take place without any external input to the system. It can also be defined…

Q: Complete the thermodynamics table for the processes shown. Reaction or Process Spontaneous? Sign…

A: A spontaneous reaction is one which favours the formation of products and results in an overall…

Q: Given the thermal chemical reactions below Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ∆H°= −26.7 kJ…

A: Enthalpy measures the heat content of a system. If change of enthalpy is positive then the reaction…

Q: 1. For the reaction at 25̊ C, find ∆G° and determine what type of reaction/process takes place. a.…

A: Gibbs energy or free enthalpy, is a quantity that is used to measure the maximum amount of work done…

Q: First Law of thermodynamics I. Calculate AU for each of the following cases & identify if the…

A: Exothermic reaction :- In a reaction the amount of heat released then the reaction is known…

Q: Given the reaction: NO2(g) NO(g) + O2(g) (H = +62 Kj), if the temperature is increased, the…

A: Given ;- NO2(g) <-----> NO(g) + O2(g) H = +62 kJ statement : if the temperature is…

Q: If 117.4 g of copper at 100.0 ℃ is added to 26.7 grams of water at 25.7 ℃, what is the final…

A: Given , 117.4 g of copper at 100.0 ℃ is added to 26.7 grams of water at 25.7 ℃

Q: Consider the reaction: 2KClO3(s)~2KCl(s)+3O2(g) At a standard state, △G for the reaction is -35kJ.…

A: The value of gibbs free energy change helps us to find if the reaction at a particular temperature…

Q: A certain reaction has a positive value of enthalpy change. Which of the following statements is/are…

Q: 2. Many manufactures produce hydrogen gas from methane gas, as in the reaction below. This reaction…

A: First we will calculate the number of moles in 2.50 kg and then calculate the amount of heat…

Q: Dessicants (drying agents) can often be regenerated by heating, although it is generally not…

Q: For a certain reaction, ΔH = -35.4 kJ/mol and ΔS = -85.5 J/K mol. Is this reaction endothermic or…

Q: Using enthalpies of formation (See the Supplemental Data), calculate ΔH° (in kJ) for the following…

Q: Calculate the enthalpy change for the reaction P4O6 (s)+ 2O2(g)= P₄O₁₀(s) given the following…

A: Enthalpy change refers to the amount of heat evolved or absorbed in a reaction which is at constant…

Q: The standard state Gibb's energy and entropy changes are known for the reaction: 2H,S(g) +…

Q: Using enthalpies of formation (See the Supplemental Data), calculate ΔH° (in kJ) for the following…

Q: Using Hess’s Law, show or describe how the given equations below can be used to calculate the…

Q: The standard enthalpy change for the following reaction is -1.55×103 kJ at 298 K. 2 Fe(s) + 10…

A: Standard enthalpy change for the given chemical reaction

Q: How much heat is absorbed in the complete reaction of 3.00 grams of SiO, with excess carbon in the…

Q: For a reaction, Delta H = -145 kJ and Delta S = 220 J. Is the reaction spontaneous? O Always O At…

A: We know ; ∆G = ∆H - T∆S When the Value of ∆G is negative , then the Reaction is spontaneous . &…

Q: . What is true about the spontaneity of a reaction? a.When the products have less enthalpy than…

A: In this question, we want to identify correct statement about spontaneity of a reaction. You can see…

Q: Consider the reaction. 2Fe2O3⟶4Fe+3O2 Δ?∘rxn=+824.2 kJ The formation of 77.0 g77.0 g of Fe…

A: Molar mass of Fe = 55.845 g/mol 4 moles of Fe = 223.38 gm Means, 223.38 g Fe forms with absorption…

Q: In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The…

A: We are given the balanced chemical equation for the preparation of NH3 as follows: HNO3(g) +…

Q: At one time, a common means of forming small quantities ofoxygen gas in the laboratory was to heat…

Q: N2(g) + O2(g)⟶2NO(g) ΔH = 180.5kJ NO(g) + 1O2(g)⟶NO2(g)ΔH = −57.06kJ 2 Calculate the ΔH…

A: Given data N2(g) + O2(g)⟶2NO(g); ΔH1 = 180.5 kJ --------------------equ (1) NO(g) +…

Q: OAttempt 1 Calculate the standard enthalpy change for the reaction at 25 C. Standard enthalpy of…

Q: A certain reaction has ΔH∘ = + 35.8 kJ and ΔS∘ = 85.5 J/K. 1. exothermic or endothermic? 2. Does…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: A chemist fills a reaction vessel with 2.62 atm nitrogen (N₂) gas, 3.76 atm hydrogen (H₂) gas, and…

Q: Calculate ΔH for the reaction NO(g) + O(g) → NO2(g) given the following information: NO(g) +…

A: Introduction The value of heat of reaction can be calculated by the application of Hess's Law.

Q: 1. When work is done on the system (+∆G) to bring it into an ordered state (-∆S) which of the…

A: Interpretation: The given question are to be solved.

Q: What is the free energy change for the process shown here under the specified conditions? T = 25…

A: We know that ∆G = ∆G° + RTlnQ ..(1) Here, Q = pH2^3*pN2^1/pNH3^2 = (0.250)^3(0.870)/(12.9)^2 =…

Q: Consider the reaction described by the chemical equation shown. 3 C₂H₂(g) → CH (1) AHxn=-633.1 kJ…

Q: The chemical reaction 2A(g) + 2B(g) + C(g) > AB2(g) +AC(I) is spontaneous at 300 K and…

Q: Which of the following processes is both exothermic (at 1 atm) and spontaneous? A) Sublimation of…

A: The process which is both exothermic and spontaneous is condensation of water at 99.5°C.

Q: Calculate the standard heat of formation of carbon disulfide (CS 2) from its elements, C(s) + 2 S(s)…

A: In this question, we will determine the standard heat of formation of CS2 ∆H°f You can see details…

Q: Calculate the enthalpy change for the reactionP4O6(s) + 2 O2(g) -----> P4O10(s)given the…

A: The given reactions are, From the above equations, it is clear equation (3) can be obtained by…

Q: For the reaction CO(g) + 3H2(g)CH4(g) + H2O(g) H° = -206 kJ and S° = -215 J/K At standard…

A: We know that a reaction equilibrium is product favored or in simple words, spontaneous, when Now,…

Q: 1. Given the following thermochemical data at 25°C and 1 atm pressure, 3 02(g) + 2B(s) → B2O3(s)…

A: Given, 3/2 O2 (g) + 2 B(s) →B2O3 (s) ∆H1°= -1264kJ O3 (g) + 2B (s) →B2O3 (s) ∆H2°= -1406 kJ 2O3…

Q: For the reaction 2HBR(g) + Cl2(g)- 2HCI(g) + Br2(g) AH° = -81.1 kJ and AS° = -1.20 J/K At standard…

Q: Consider the reaction: ICl(g) + Cl₂(g) → ICl₃(s). The ∆G° of the reaction is -17.09 kJ/mol.…

A: Given, ICl(g) + Cl₂(g) → ICl₃(s) ∆G° = -17.09 kJ/mol.

Q: Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free…

Q: For the reaction: N2(g) + 2O2(g) + 16.2 kJ ➜ 2 NO2(g) As nitrogen reacts with oxygen, the heat of…

A: Nitrogen dioxide = N2O Heat of formation of N2 = 0 kJ Heat of formation of O2 = 0 kJ If heat is…

Q: 2. The overall reaction in a commercial heat pack can be represent 4Fe(s) + 30₂ (g) 2Fe₂O3 (s) How…

A: 2) Given, 4Fe(s) + 3O2(g) ➝ 2Fe2O3 ∆H = -1652 kJ moles of Fe2O3 produced = 1.00 mole Amount of…

Q: 1. The standard enthalpy changes for the formation of aluminium oxide and iron (III) oxide are 2…

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

Q: Consider the following reaction: CO (g) + 2 H2 (g) - CH;OH (g) AH= -907 k Calculate the amount of…

Q: Part A. In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen…

A: HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ From this data we get that , When 4 mole Hydrogen…

Q: Calculate the free energy change for the formation of one mole of ammonia from its elements under…

A: The formula that can be used in the solution is : ΔG° = ΔG°f(products) - ΔG°f(reactant)

Q: Given the following reactions: 2S(s) + 3O2(g) → 2SO3(g) ΔH = -790 kJ S(s) + O2(g)…

A: Hess's law is defined as amount of energy released or absorbed is same wheather the reaction take…

Question

100%

The standard state Gibb's energy and entropy changes are known for the
reaction:
2H, S(g) + 30,(g)=2H20(g) + 2SO2(g)
What is the standard state enthalpy change for the reaction at 25 C?
120 kJ
52 J
AGº
ASº
Mole
Mole K
-68 kJ/mol
154 kJ/mol
104 kJ/mol
O -119 kJ/mol

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

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

Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4: Ni(s)+4CO(g)Ni(CO)4(g) This reaction is exploited in the Mond process in order to separate pure nickel from other metals. The reaction above separates nickel from impurities by dissolving it into the gas phase. Conditions are then changed so that the reaction runs in the opposite direction to recover the purified metal. (a) Predict the sign of S for the reaction as written above. (b) Use tabulated thermodynamic data to calculate H, S , and G for the reaction. (c) Find the range of temperatures at which this reaction is spontaneous in the forward direction.
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
What is the second law of thermodynamics? For any process, there are four possible sign combinations for Ssys and Ssurr. Which sign combination(s) always give a spontaneous process? Which sign combination(s) always give a non-spontaneous process? Which sign combination(s) may or may not give a spontaneous process?
Enthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.
What is the third law of thermodynamics? What are standard entropy values, S, and how are these S values (listed in Appendix 4) used to calculate S for a reaction? How would you use Hesss law to calculate S for a reaction? What does the superscript indicate? Predicting the sign of S for a reaction is an important skill to master. For a gas-phase reaction, what do you concentrate on to predict the sign of S? For a phase change, what do you concentrate on to predict the sign of S? That is, how are Ssolid, Sliquid, and Sgas related to one another? When a solute dissolves in water, what is usually the sign of S for this process?
The reaction shown below is involved in the refining of iron. (The table that follows provides all of the thermodynamic data you should need for this problem.) 2Fe2O3(s)+3C(s,graphite)4Fe(s)+3CO2(g) (a) Find H for the reaction. (b) S for the reaction above is 557.98 J/K. Find S° for Fe2O3(s). (c) Calculate G for the reaction at the standard temperature of 298 K. (There are two ways that you could do this.) (d) At what temperatures would this reaction be spontaneous? Compound Hf (kJ mol-1) S° (kJ mol-1) Gf (J mol-1 K-1) Fe2O3(s) -824.2 ? -742.2 C(s, graphite) 0 5.740 0 Fe(s) 0 27.3 0 CO2(g) -393.5 213.6 -394.4.83
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is equal to 358 J/K. Use this value and data from Appendix 4 to calculate the value of S for CF4(g).
Determine whether each of the following statements is true or false. (a) An exothermic reaction is spontaneous. (b) When G° is positive, the reaction cannot occur under any conditions. (c) S° is positive for a reaction in which there is an increase in the number of moles. d) If H° and S° are both negative, G° will be negative.
For each process, tell whether the entropy change of the system is positive or negative, (a) A glassblower heats glass (the system) to its softening temperature, (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)
For the reaction at 298 K, 2NO2(g)N2O4(g) the values of H and S are 58.03 kJ and 176.6 J/K, respectively. What is the value of G at 298 K? Assuming that H and S do not depend on temperature, at what temperature is G = 0? Is G negative above or below this temperature?