What is the free energy change in kJ/mol for the process below at 42.9 °C when the concentration of A =0.49 M, B = 0.84 M and C = 0.35 M? 2 A(aq) ⇋ 2 B(aq) + C(aq)     ΔG° = 12.5 kJ/mol Report your answer to two decimal places and do not include units

Q: Consider the oxidation of a generic metal MM into a metal oxide as shown in the reaction.…

A: Data :- ∆H°rxn = −3.733 kJ/mol  ∆S°rxn=11.54 J/(mol⋅K) T = 298K  ∆G=?  Equilibrium constant,K=?

Q: The change in standard free energy (i.e. ΔG°) for a particular reaction has a value of −34.9 kJ/mol…

A: ΔG° = -34.9 KJ/mol = -34.9×103 J/mol ΔG° = -34900 J/mol Temperature (T) = 34.6°C = (34.6+273.15)K T…

Q: At 961. K, ΔGo equals -77.2 kJ for the reaction, N2O4(g) ⇌ 2 NO2(g).   Calculate the value of…

A: The relationship between deltaG°(the free energy change) and K (the equilibrium constant) is…

Q: Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Refer to the AG°f…

A: In the given question we have to calculate the standard change in Gibbs free energy for the…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction at 20.0 °C is -50.9 kJ.…

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Q: Using ΔG ̊f Calculate the K for N2 + 3H2 → 2NH3 at 25 ̊C ΔG ̊rxn = -33.32 kJ

A: To calculate the equilibrium constant ( K ) for the reaction N2​+3H2​→2NH3​ at 25°C using the Gibbs…

Q: Chemistry please answer in tipping format

A: Given chemical equation SnO2​(s)+2CO→Sn(s)+2CO2​(g)ΔG0=−194KJ1) in this equation divide the above…

Q: Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith…

A: The problem is asking us to calculate the enthalpy change (ΔH⁰) and entropy change (ΔS⁰) for the…

Q: Which of the following changes in Gibbs free energy represents a spontaneous reaction? O AG(-) O…

A: To solve this problem we have to explain about the type of reaction according to value of ∆G .

Q: Calculate ∆G  (in kJ) at 35.4oC for a reaction that has Keq = 119

A: Using Keq we can calculate ∆G at particular temperature.

Q: The standard reaction free energy AG = -1181. kJ for this reaction: 4 H2O2(1) + PbS(s)→PbSO4(s) + 4…

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Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: When free energies (useful work) are estimated under standard conditions (1 atm pressure and 273.15…

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: ST3D.3- At constant temperature and pressure, what is the minimum mass [in g] of glucose needed for…

A: Answer: Value of gibbs free energy change is always equal to non-expansion work and over here…

Q: Calculate the standard entropy, Δ?∘rxn, of the reaction at 25.0 ∘C using the table of thermodynamic…

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Q: Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.…

A: Recall the given reaction,                                      M2O s ↔ 2 M s + 12 O2 g ∆Gf° kJmol :…

Q: The standard reaction free energy AG = 150. kJ for this reaction: 6C1₂(g) + 2Fe₂O3(s) 4 FeCl3(s) + 3…

A: ∆G is an extensive and additive thermodynamics properties. ∆G of reverse reaction is the -ve of ∆G…

Q: For the following reaction at 276°C, calculate Keq. 2 A (s)  +  B (g)  →  C (g)  +  D (s) ΔS°  =…

A: Equilibrium constant  is defined as the product of concentration of products divided by the product…

Q: The equilibrium constant for the reaction2Fe3+(aq) + Hg22+(aq) ⇌ 2Fe2+(aq) + 2Hg2+(aq)is Kc =…

A: The ΔGo at this temperature is determined by using following equation,

Q: ΔG° = 91.7 kJ/mol at 25°C for the following process. Which of the following statements is correct…

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Q: Calculate the standard change in Gibbs free energy, AGxn, for the given reaction at 25.0 °C. Consult…

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Q: What is the ΔGo for the following reaction from the equilibrium constant at the temperature given?

A: ΔG°=−RTlnK Temperature = 900°C                          = 900+ 273 = 1173 K  Equilibrium…

Q: For the reaction A (g) → 2 B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298…

A: The question is based on the concept of chemical thermodynamics & equilibrium. we need to…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: Gibbs free energy  ∆G = ∆G° + RTln Q formula used

Q: Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith…

A: The problem is asking us to calculate the enthalpy change (ΔH⁰) and the entropy change (ΔS⁰) for the…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

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Q: A student determines the value of the equilibrium constant to be 4.03×10-18 for the following…

A: Solution-  ∆Gorxn is given as,-∆Gorxn=-RT ln Keq.=-8.314 Jmol-1K-1×298K× ln( 4.03×10-18)=-8.314…

Q: Calculate ∆G  (in kJ) at 35.4oC for a reaction that has Keq = 105

A: Given: Temperature = 35.4 oC And Keq = 105

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

A: In a chemical reaction   ΔG° =∑ΔG°Products   -  ∑ ΔG°reactants. For given reaction…

Q: In a typical cold pack (used for sports injuries), a salt such as ammonium nitrate is kept in a…

A: Dissolution of ammonium nitrate in water is given by, NH4NO3(s)→H2O(l) NH4+(aq)+NO3-(aq)   ∆H=+25.09…

Q: The equilibrium constant for a particular reaction has a value of 7.40 × 10−4 at a temperature of…

A: Equilibrium constant, K = 7.40 × 10-4   Temperature , T = 24.4°C = ( 24.4 + 273)K = 297.4 K…

Q: Discuss the spontaneity of each process in the following scenarios, based on the use of the Gibbs…

A: The spontaniety of Reaction depends upon the sign of ∆G value for the reaction . The reaction is…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction at 25.0 °C is 56.5 kJ.…

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Q: For the following reaction at 276°C, calculate Keq. 2 A (s)  +  B (g)  →  C (g)  +  D (s) ΔS°  =…

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Q: What is AS° (rxn) for the reaction 2 A→ 3 B if S° (A)=120.0J/mol · K and S° (B) = 200.0 J/mol ·K?

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Q: – 10 For a certain chemical reaction, the equilibrium constant K = 4.5 × 10 at 5.00 °C. Calculate…

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Q: -4 For a certain chemical reaction, the equilibrium constant K = 1.9 × 10 at 5.00 °C. Calculate the…

A: Given that, K=1.9×10-4 T=5.00℃ = (5.00+273) K = 278 K ∆G°= ?

Q: Use the table of thermodynamic values to calculate the value of ΔG°rxn at 25.0 °C for the reaction…

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Q: What is the Gibbs Free Energy of the following reaction: CH4(g) +20₂(g) + CO₂(g) + 2H₂O(g) Substance…

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Q: Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the…

A: Concentration of all ions = 0.0008 M  Temperature, T = 298 K F = 96485 C/mol R = 8.314 J.mol-1.K-1…

Q: Calculate AG° and K, at 25 °C for the reaction 2 HBr(g) + Cl2(g) → 2 HCI(g) + Br,(t) Is the reaction…

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Q: Using the following data to calculate the value of ΔvapH° (in units of kJ/mol) of water at 365 K:…

A: The given values are: ∆vapHo373 = 40.7 kJ/mol ∆vapHo365 = ?? (To be calculated) Cp(g) = 33.6…

Q: For the reaction A (g) 2 B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298 K…

A: ∆G = ∆G° + RTlnQ ∆G = - RTlnK + RTlnQ K = equilibrium constant Q = reaction quotientR = gas…

Q: At  25 ∘C , the equilibrium partial pressures for the reaction 3A(g)+4B(g)↽−−⇀2C(g)+2D(g)   were…

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Q: The reaction                         C6H12O6 + 6O2  →  6CO2 + 6H2O ΔHo = −1072 kJ/mol and ΔSo =…

A: For the given reaction,  ∆H° = -1072 kJ /mol = -1072 × 103 J mol-1 ∆S° = 578 J K-1 mol-1 T = 37 ℃ =…

Q: Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases…

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Q: The equilibrium constant for a particular reaction has a value of 4.84 × 10−5 at a temperature of…

A: Equilibrium constant (k) = 4.84×10-5 Temperature (T) = 20.1°C = (20.1+273.15) K T = 293.25 K ΔG° = ?…

Q: Use the data below to calculate AG°rxn for the reaction: H, (g) +CO,(g) – H,0(g) +CO(g) Data: H, (g)…

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