What is ΔG° at 500.0 K for the following reaction?  You need to show your works. Zn(s) + H2O(g) →ZnO(s) + H2(g) Substance ΔH°f (kJ/mol) at 298 K S° (J/(mol∙K)) at 298 K Zn(s) 0 41.6 H2O(g) –241.8 188.7 ZnO(s) –350.5 43.7 H2(g) 0 130.6 A. 92.0 kJ B. –136.7 kJ C. –80.7 kJ D. –92.0 kJ E. 80.7 kJ

Q: Calculate the ASuni for the following reaction at 25°C in J/mol K. 2CH3OH(I) +302(g) → 2CO2(g) +…

A: Entropy is the spreading out of energy. Energy tends to spread out as much as possible. Therefore…

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: 13) Calculate AG° spontaneous in each case? for the reaction above at a) -50.0 °C and at b) 675 °C.…

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Q: 10. Consider the reaction: Ag+ (aq) + Cl- (aq) AgCI (s) Given the following table of thermodynamic…

A: Given ; reaction

Q: Calculate the ΔG° (kJ/mol) for the following reaction at 152 °C, using the following data.  Eneter…

A: Answer: -2085.472485 kJ/mole is the value of ∆G°rxn at 152°C

Q: SO3 ​(g) + H2​O (l) ------> H2​SO4​ (aq) ΔS° =  ______J/K

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Q: For the reaction C(s) + H20 (g) – CO(g) + H2 (g) AH° = 131.3 kJ/mol and AS° = 133.6 J/mol-Kat 298 K.…

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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: Which of the following reactions correctly depict reactants and products in the correct state to…

A: In the reaction, states of matter was written as a subscript to the molecules which takes part in…

Q: Which of the following changes will always be true for a spontaneous reaction?  +ΔG  –ΔG  +ΔS…

A: The spontaneous reaction means the reaction which occur without intervenation at given set of…

Q: What is the standard free-energy change ΔG° at 25°C for the following reaction? See the Supplemental…

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Q: a) image attached b) Calculate ΔG∘ at 296 ∘C c) tell whether the reaction has an equilibrium…

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Q: What is the free energy change in kJ/mol for the process below at 19.97 °C when the concentration of…

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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: Determine the equilibrium constant for the following reaction at 298 K to one decimal point. SO3(g)…

A: We know that change in the standard Gibbs free energy is equal to the product of gas constant ,…

Q: What is ΔG° at 25 ºC for a process that has ΔH° = −35.4 kJ/mol and ΔS° = −153 J/mol·K? 45.6 kJ/mol…

A: Given: ΔH° = −35.4 kJ/mol  ΔS° = −153 J/mol·K Temperature T =  25 ºC = 273 + 25 = 298 K

Q: For the reaction 2 A B, the value of Kc = 4.50, at 100oC. Determine the value of ∆G, in kJ/mol for…

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Q: A) AG becomes less negative and the reaction becomes less spontaneous. B) AG becomes more negative…

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Q: Carbon tetrachloride, an important industrial solvent, is prepared by the chlorination of methane at…

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

A: Entropy- Entropy is a thermodynamic property. Entropy determines spontaneity of process.…

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: Consider the reaction:CH3OH( g)<--------->CO( g) + 2 H2( g)Calculate ΔG for this reaction at…

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Q: This industrial chemical reaction process generates nitrogen monoxide, an important component in the…

A: The question is based on the concept chemical thermodynamics.   We have been given  chemical…

Q: Use thermodynamic values in the table provided to calculate the ΔG for the following process in two…

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Q: Directions: Given the AH° and AS°, Calculate the AG° values for the following reactions and indicate…

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Q: Calculate the ΔS°rxn of the following reaction at 223°C and standard pressure. =_____J/mol•K

A: The reaction given is,

Q: Calculate the ΔGo for the following equation.   Sb4O6(s) + 6C(graphite) ⟶ 4Sb(s) + 6CO(g) Group…

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Q: Calculate ΔG0reaction in kJ/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)…

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Q: What is the free energy change in kJ/mol for the process below at 42.9 °C when the concentration of…

A: Given that:  ΔG° = 12.5 kJ/mol [A] = 0.49 M [B] =  0.84 M [C] = 0.35 M T = 42.9 °C = (42.9 + 273) K…

Q: Calculate ΔG°rxn at 298 K for the reaction:I2(g) + Cl2(g)<-------->.2 ICl(g) Kp = 81.9

A: Gibbs free energy It is represented by the symbol ∆G. Change in the Gibbs free energy is defined as…

Q: Consider the reaction given below. H2(g) + F2(g) 2 HF(g) (a) Using thermodynamic data from the…

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Q: For each reaction, predict the sign and find the value of ΔS°:

A: It’s given below :

Q: Use the data shown below, to calculate AH°rxn and AS°rxn at 25°C for the following reaction: 3 H₂(g)…

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Q: Consider the following system at equilibrium where AH = 108 kJ, and K = 0.0129, at 600 K: COC1₂(g) →…

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Q: What is the standard free-energy change ΔG° at 25°C for the following reaction? See the Supplemental…

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Q: Determine ΔG0 at 298 K for N2(g) + 3 H2(g) <---> 2NH3(g) given Substance ΔH0f (kJ/mol)…

A: The given reaction is, N2(g) + 3H2(g) → 2NH3(g) The enthalpy change of the reaction can be…

Q: Calculate ΔS^0reaction in J/mol at 298.15 K given N2(g)+O2(g)→2NO(g)…

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

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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° =…

Q: The equilibrium constant for the reaction below decreases from 12810.0 at 520.0°C to 29.0 at…

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Q: Calculate Δ S° for the following reaction.  N 2( g) + 2 O 2( g) → 2 NO 2( g) a: -121.5 J/K b: 636.5…

A: The formula used to get the Δ S° for any reaction is given as - Δ S°rxn = Δ S°pdt - Δ S°rct