rank the following reactions from smallest to largest equilibrium constant (K) at 298K? reaction 1: Fe2O3(s)+3CO(g)->2Fe(s)+3CO2(g), ∆G°=-28.0kJ reaction 2: Ca CO3(s)->CaO(s)+CO2(g), ∆G°=+131.1kJ reaction 3: 2Hg(g)+O2(g)->2HgO(s), ∆G°=-180.8kJ reaction 4: 3O2(g)->2O3(g), ∆G°=+326kJ the answer is suppose to be (reaction 1, reaction 3, reaction 2, reaction 4) but I don't understand how this is possible. I was told to use Keq=e^-∆G° / RT. The values I got for the reaction are: 1.0113, 0.94846, 1.0757 and 0.87671, but I don't know how 1.0113<1.0757<0.94846< 0.87671

Q: For the reaction: N2O4(g) ó 2 NO2(g)​Kp = 0.113 at 25.00 oC. The standard state free energy change…

A: Given: N2O4(g) &lt;---&gt; 2 NO2(g)       ​Kp = 0.113  at 25.00 oC. ∆G° = 5.40 kJ /mol

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

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Q: Calculate ΔG° rxn for the reaction below given the Gibbs free energies of formation.

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Q: What is the equilibrium constant for a reaction at temperature 59.3 °C if the equilibrium constant…

A: Given: Initial temeperature(T1)=25.70C=(25.7+273)K=298.7 K Final temperature(T2)=59.3 °C=(59.3…

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: What is the equilibrium constant for a reaction at temperature 58.7 °C if the equilibrium constant…

A: Given,  T2 = 58.7 + 273 = 331.7  K T1 =273 + 21.1 = 294.1 K K1 = 27.1 □H = 14.7 kJ/mol Using  Von't…

Q: In a reaction, 1.00 mole of H2 is produced at a constant pressure of 1.00 atm and at 298 K (1 L atm…

A: Therefore, ΔE in this reaction is +483.6 kJ.Explanation:The equation for calculating ΔE is:ΔE = ΔH -…

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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 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: The equilibrium constant (KP) for the reaction is 4.24 at 800 K. (a) Calculate ∆G° for the reaction.…

A: T = 800 K By using this formula we can calculate the Value of ∆G°

Q: What is the equilibrium constant at 25o C for the reaction 2 CO(g) + O2(g) ⇌ 2 CO2(g) given the…

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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: CaCO3(s) → CaO(s)+CO2(g)CaCO3(s) → CaO(s)+CO2(g)      Calculate the value of the equilibrium…

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Q: None

A: The relationship between gibbs energy (ΔGo), enthalpy (ΔHo) and entropy (ΔSo) is given by the…

Q: For the reaction: 2 NO2(g) ó N2O4(g)​Kp = 8.85 at 25.00 oC. The standard state free energy change…

A: Given, Kp of the reaction is 8.85 Temperature, T = 25 oC = 298K Standard free energy, ∆Go= -5.40…

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: 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: Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction : N2(g) + O2​(g)…

A: The relationship between equilibrium constants at two different temperatures is given as :

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: What is the free energy change when silver chloride form at 2000.0 K? Ag+ (aq)  +  Cl–   (aq)     →…

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Q: Calculate the equilibrium constant at 250.0 °C.

A: Given data :

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: For the reaction: C (s, graphite) + TiO (s) + 2Cl (g) ↔ TiCl4 (g) + CO2 (g) (a) demostrate that, at…

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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: If the reaction is spontaneous calculate the equilibrium temperature

A: For a spontaneous reaction, ∆Go ≤0 To calculate the equilibrium temperature, put ∆Go = 0   From…

Q: We start with a pure sample of A(g). The following equilibrium is established: 2 A(g) B(g) + C(g)…

A: Given: Total pressure (PT) is 8.56 atm. Partial pressure of A is 5.43 atm.

Q: Calculate the deltaH of formation ZnSO4 (s) from the following data: Zn (s) + S (s) --> ZnS (s)…

A: The ΔH of formation ZnSO4 can be determined using Hess’s Law. According to Hess’s Law, if a reaction…

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: Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction…

A: Given data, ∆H° = 180.50 KJ = 180500 J ∆S° = 24.77 J/K Temperature (T) = 25°C = (273+25) = 298 K

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: For a spontaneous endothermic chemical reaction with ArxnH°= +20.6 kJ/mol, the equilibrium constant…

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Q: Calculate the missing data in the following table. Compound ΔHvap (kJ/mol) ΔSvap [J/(mol·K)]…

A: The formula relating ∆Hvap and ∆Svap is: ∆Svap = ∆Hvap  Tb where Tb = Boiling point temperature in 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: For the decomposition of silver oxide, at 298 K and 1 atm, according to the chemical equation:…

A: We have to calculate the ∆G and temperature

Q: Consider the following system at equilibrium where AH° = -87.9 kJ, and Kc = 83.3, at 500 K: PC13 (9)…

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Q: For the reaction Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) = 206 J/K The equilibrium constant…

A: For the reaction, Ca(OH)2(aq) + 2HCl(aq) ----&gt; CaCl2(s) + 2H2O(l) Enthalpy change (∆H°) = -30.2…

Q: 10) Consider the following reaction HCN (g) +2 H: (g) → CH:NH: (g) AH°= -158.0 kJ; AS°= -219.9 J/K…

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Q: SiH4 (g) + 2 O2 (g) -> SiO2 (s) + 2 H20 (l) at 25ºC; where ΔН°rxn = -1 516 kJ and ΔSºrxn = -432.8 J…

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Q: NO2

A: Given values - Kp = 4.15 × 10^-50 T = 523K

Q: alculate the change in free energy for the following reaction at 372 K: J (s)  →  L (s)  +  Q (g)…

A: To calculate the free energy change at 372 K when partial pressure of Q is PQ = 0.0628 atm. Given…

Q: When heated above 840°C, calcium carbonate decomposes, releasing carbon dioxide gas and leaving…

A: ∆G° of a process can be calculated from ∆H° , ∆S° and temperature by using the formula ∆G° = ∆H° -…

Q: Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH (g) →3 Ni(s) + N,(g) + 3 H,O(g) K If AH° =…

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Q: The standard Gibbs free energy change is 2.60 kJ/mol for the reaction at 25.0oC: H2(g) + I2(g) →←…

A: Given: H2(g) + I2(g) →← 2HI(g);    ∆Gorxn = + 2.60 kJ/mol

Q: Calculate the standard free energy ΔGo (in kJ/mol) knowing that the equilibrium constant Kc is…

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Q: Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N₂(g) +…

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Q: For the reaction CO₂(g) + H₂(g) → CO(g) + H₂O(g) = : 41.2 kJ and AS⁰ = 42.1 J/K ΔΗ° The equilibrium…

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