Consider the reaction: C6F6(g) <--> 3C2F2(g). Given that ΔH° = 591.1 kJ/mol and ΔG° = 495.4 kJ/mol at 25°C, calculate ΔS° Group of answer choices 0.261 kJ/K 3.83 kJ/K 3.11 kJ/K 321 J/K

Q: What is the free energy change at 25°C for the reaction below, if ΔGfo(CH4(g) = -50.790 kJ/mol,…

A: The standard Gibbs free energy change for the formation of substances in their standard state is…

Q: Consider this reaction at 298 K: CO2 (g) + H2 (g) ⇌ CO (g) + H2O (g) Calculate ΔGrxn under the…

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Q: What is ΔG°rxn in kJ/mol for the following reaction at 537.8 Kelvin? Please report 2 decimal places,…

A: The enthalpy of a reaction is the amount of heat energy gained or released during the course of the…

Q: a) Calculate AGxn for the reaction (AHrxn=572 kJ; ASrxn° = 179 J/K).

A: We know ∆Gorxn = ∆Hrxno - T∆Srxno . For a reaction to be spontaneous ∆G should be -ve . At…

Q: For a given reaction, the ΔS°rxn is 239.9 J/mol*K and the ΔG°rxn is -212.7 kJ/mol at 298 K. What is…

A: In the given question we have to calculate the change in free energy at 580 K , assuming that…

Q: chapter 12:  9) What are ΔH°rxn, ΔS°rxn, and ΔG239.0 K for the following reactions at 239.0 K?…

A: Given Temperature = 239.0°K Compound ΔHºf (kJ/mol) Sº (J/mol • K)  H2S(g)  –20.17  205.6…

Q: Consider the reaction 2 NO2(g)  N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and Gf NO2(g) = 51.3…

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Q: Consider a reaction occurring at 132°C that has a ΔH° of 449 kJ/mol and a ΔS° of -326 J/(mol⋅K).…

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Q: The overall reaction for the corrosion of iron (rusting) by oxygen is…

A: Solutions The overall reaction for the corrosion of iron (rusting) by oxygen is…

Q: Calculate T (in K) given ΔG0= -89.9 kJ/mol and ΔH0= 83.1 kJ/mol and ΔS0= 669 J/mol K

A: Given ΔG° = -89.9 kJ/mol ΔH° = 83.1 kJ/mol ΔS° = 669 J/mol K

Q: 8) For the reaction at 298 K, 2NO2(g) --> N2O4(g) The values of ΔH=−58.03 kJ and ΔS=−176.6 J/K. What…

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Q: For a particular reaction at 225.9 °C, Δ?=−1076.67 kJ/mol , and Δ?=785.08 J/(mol⋅K) . Calculate ΔG…

A: T = 225.9 °C = 498.9 K ΔG = -1076.67 kJ/mol ΔS = 785.08 J/(mol⋅K) = 0.78508 kJ/(mol⋅K) ΔG at -22.8…

Q: If Keq for the reaction below at 225°C is 1.87 x 1010, calculate ΔS°rxn. B2 (g)  +  2 A (g)  →  2…

A: The randomness of the system is known as entropy of the system.

Q: 11. What is the ΔHº-value for the dissolution of NaOH (s) to yield 1.00... m NaOH (aq), given:…

A: Given data   Na (s) + 12 O2 (g) + 12 H2 (g) → NaOH (s)                ΔHfº = -425.9 kJ/mole   Na (s)…

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

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Q: Given that ΔG0f  for SF6 = -1105 kj/mol, and  ΔG0reaction = -374 kj/mol, what is ΔG0f  for SF4 in…

A: Given:  ΔG0f for  SF6 = -1105 kJ/mol ΔG0f for  F2 = 0 kJ/mol ΔG0reaction = -374 kJ/mol

Q: For the process: HXO2(g) ⇌ HXO2(l) if ΔH° is -39.04 kJ/mol and ΔS° is -111.74 J/(mol ∙ K). What is…

A: The normal boiling point is the temperature at which a liquid's vapour pressure becomes equals to…

Q: A reaction has the following thermochemical values at 272.15 K: ΔH = -189.3 kJ mol-1 ΔS = -166.0 J…

A: Given-&gt; Temperature (T) = 272.15 K ∆H = -189.3 kJ.mole-1 = -189300 J.mole-1(1KJ=1000J) ∆S =…

Q: Consider the reaction that occurs during the Haber process:N2( g) + 3 H2( g)¡2 NH3( g)The…

A: The laboratory synthesis of ammonia by the treatment of nitrogen gas on hydrogen at moderately…

Q: ΔG° = -RTln(K)    =>-3.9 × 105 J/Mol.  = - 8.314 J/K .Mol × 298K ln (K)   By Solving K = 9.77×…

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Q: What is the value of ΔG when ΔH = -24 kJ and  ΔS = -44 J/K at 283 K?

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Q: What is ΔG°rxn in kJ/mol for the following reaction at 406 Kelvin? Please report 2 decimal places,…

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Q: Consider a process with ∆H = -89.8 kJ and ∆S = -151 J/K.  At what temperature will this process be…

A: The objective of the question is to find the temperature at which the process will be at…

Q: Consider the reaction: Co2(g) + H2(g)→CO(g) + H,0(g) Using standard thermodynamic data at 298K,…

A: ∆G°rxn = ∆G°f(products ) - ∆G°f(reactants )

Q: What is K for a reaction if /\G° =-178.6 kJ/mol at 25 °C (or 298 K)? (R = 8.314 J/mol • K)

A: Information of question

Q: reaction has the following thermochemical values at 273.15 K: ΔH = -184.8 kJ mol-1 ΔS = -166.6 J…

A: Given,  ΔH = -184.8 kJ mol-1 ΔS = -166.6 J mol-1K-1 Temperature = 273.15 K

Q: Given the balanced reaction 4A = B + 3C, what is the ΔG of the reaction if:   ΔHf (J/mol) ΔS…

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Q: Keq

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Q: 2 A (g) + B (g) -> 2 C (s) ΔHº = ‒75.0 kJ ΔSº = ‒150.0 J/K ΔGº= -30.3 kJ iv. 0.100 atm of A,…

A: Given:- For this reaction :- 2 A (g) + B (g) ⇒ 2 C (s) ΔHº = ‒75.0 kJ  ΔSº = ‒150.0 J/K  ΔGº= -30.3…

Q: Calculate the ∆G in kJ/mol for a reaction at room temperature (~25.00°C) that has a Keq = 1000.0.…

A: We have to calculate the ∆G.

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

A: According to Thermodynamics,  ∆G&gt;0 = non spontaneous ∆G&lt; 0 = spontaneous ∆G = 0 , At…

Q: Using only the data given below, determine ΔG⁰ for the following reaction: NO(g) + O(g) → NO₂(g)…

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Q: Consider the reaction:             N2(g) + 3H2(g) --> 2NH3(g) where ΔH = -15.0 kcal/mol and ΔS =…

A: Given reaction; N2(g) + 3H2(g) --&gt; 2NH3(g) where, ∆H = -15.0 Kcal/mol and, ∆S = -35.0 cal/mol.K…

Q: ΔGo' for the isomerization reaction glucose-1-phosphate (G1P) ⇋ glucose-6-phosphate (G6P) is -7.10…

A: We have to predict the ratio of [G1P] to [G6P]

Q: The synthesis of the pesticide thionyl chloride (OSCl2) proceeds according to the following…

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Q: Consider the following reaction: 2C(s) + 2H2(g) → C2HA(g); A,H° = 52.47 k); A,S° = -53.5 J/K at 298…

A: Given equation: 2C +2H2 →C2H4 ∆G=∆Go+RTlnKeq here ∆Go=∆Ho-T∆S0 ∆Go=52.47 x 1000 -298(-53.5)…

Q: CaCl2 (MM = 110.98 g/mol) is used as road salt in the winter to minimize the accumulation of ice on…

A: On adding dissolving CaCl2, the temperature will change from initial value. Heat absorbed by water…

Q: For a particular reaction at 128.2 °C, AG = 190.07 kJ/mol, and A.S = 658.97 J/(mol K). Calculate AG…

A: GIBBS FREE ENERGY: The change in the Gibbs free energy, when a reaction occurs at a standard…

Q: Sodium carbonate can be made by heating sodium bicarbonate:          2NaHCO3(s) ® Na2CO3(s) + CO2(g)…

A: Given : reaction      ∆G° = 33.1 kj/mol      ∆H° = 128.9 kj/mol      T = 298 k  Tip:         ∆G° =…

Q: The value of ΔH° for the reaction below is −5314 kJ.  The amount of heat that is released by the…

A: Balanced chemical equation: 2C4H10(g) + 13O2(g)  → 8CO2(g) + 10H2O(l)      ΔH° =  −5314 kJ From the…

Q: Calculate ΔS° for each of the three following reactions using the data provided below.

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Q: A reaction has the following thermochemical values at 283.15 K: ΔH = -183.3 kJ mol-1 ΔS = -160.6 J…

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Q: Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = −5.4 kJ/mol at T = 25°C and PA = PB = 1 atm and…

A: For the given reaction: 2A(g) + B(g) → 2C(g)   ΔG° = −5.4 kJ/mol T = 25°C = 25+273 K = 298 K PA = PB…

Q: What is the equilibrium constant at 25.00°C for the reaction below? Be sure to use enough…

A: The relationship between change in standard Gibbs energy, ∆G° and equilibrium constant, K is  ∆G° =…