Calculate deltaG, K, and E at 298 K for the reaction, v and the following concentrations: 2Br -(aq) + Cl2(g) → Br2(l) + 2Cl -(aq) given E○= 0.300 [Br -]= 0.10 M, PCl2 = 0.50 atm, and [Cl-] =0.010 M.

Q: For the reaction NH,NO3(aq)N20(g) + 2H2O(1) AH° = -149.6 kJ and AS° = 99.9 J/K The equilibrium…

A: According to Gibbs Equation ∆G° = ∆H° - T∆S° And also ∆G° =-RTlnKeqm Thus we calculate equilibrium…

Q: For lithium-ion battery reaction: Li-C6 + CoO2  LiCoO2 + C6, Eº = ~4 V, what would be the change of…

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Q: 2. Find the value for the equilibrium constant, K, at 25 °C (298 K) for the following reaction. The…

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Q: For the reaction 2N2(g) + O2(g)-2N,0(g) AH° = 164.2 kJ and AS° =-148.5 J/K The equilibrium constant…

A: The Gibbs free energy and the equilibrium constant are related by the following equation: Where ∆Go…

Q: At 355 K, AG = -5.7 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are…

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Q: For the reaction 2NO(g) + O2(g)-2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium…

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Q: Given the information A+ B 2D AH = 761.8 kJ AS = 305.0 J/K %3D C D AH° = 413.0 kJ AS = -164.0 J/K…

A: Consider the target equation as; A + B → 2 C      Now, consider the given equations as follows; A +…

Q: For the reaction 2H,02)2H,0(1) + O2(g) AH° = -196.0 kJ and AS° = 125.7 J/K The equilibrium constant…

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Q: Determine the equilibrium constant of the following reaction at 298 K +2Fe3+ + Sn 2FE2+ Sn4 .From…

A: According to electro chemical series,  which metal has higher reduction potential,  reduces itself…

Q: 2. Find the value for the equilibrium constant, K, at 25 °C (298 K) for the following reaction. The…

A: Given that -               Temperature =298K       Free energy (∆G°)= -13.6 kJ…

Q: Consider the reaction shown here occurring at 25°C. A(s) + B*(aq) → A*(aq) + B(s) AG = -14.0 kJ…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

Q: A student determines the value of the equilibrium constant to be 2.05x107 for the following…

A: Given, The equilibrium constant (Keq) = 2.05 x 107. The no. of moles of Fe(s) = 1.80 moles…

Q: 3. Assuming AH° and AS° do not change with temperature, calculate the thermodynamic equilibrium…

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Q: For the reaction S(5,rhombic) + 2C0(g)SO;(g) + 2C(5.graphite) AH° = -75.8 kJ and AS° = -167.6 J/K…

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Q: For a spontaneous reaction, the AG'rn must have a sign that is v and the magnitude of K must be…

A: Given : Spontaneous Reaction  To find: Sign of ∆G° and magnitude of k Solution: There are generally…

Q: The decomposition of a generic diatomic element in its standard state is representdd by the equation…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Consider the corrosion of copper at 25 C using the overall reaction Cu(s) + 0.5 O2(g) + 2 H3O+(aq) →…

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Q: The reduction of stannous sulphide by hydrogen takes place as follows: SnS(s) + H2(g) 2 Sn(1) +…

A: The relationship between equilibrium constant and temperature under two different conditions is…

Q: A student determines the value of the equilibrium constant to be 1.91x107 for the following…

A: Ans given below

Q: Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the…

A: Given,  N2(g) + 3H2(g) ---------> 2NH3(g)  All gases have a pressure of 14.63 mmHg.  PN2(g) =…

Q: At 355 K, AG = -5.7 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are…

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Q: Calculate the standard entropy, ASn, of the reaction at 25.0 °C using the table of thermodynamic…

A: From any reaction we can calculate the entropy change and Gibbs free energy change of the reaction .

Q: Determine equilibrium constant for the following reaction under standard state.        A (g)  +  B…

A: The reaction taking place is given as, => A (g) + B (g) ----> C (g) + 1.90 KJ  Given : Entropy…

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: Given the included data, calculate AG° and K at 298 K for the oxidation of nitrite 1on to nitrate…

A: Change in standard Gibbs free energy and equilibrium constant calculation:

Q: The standard free energy of formation of ammonia is -16.5 kJ/mol. N2 (g) + 3H, (g) = 2NH,(g) What is…

A: Formula  ∆Gr° = -2.303RT log K  -16.5 x 103 J = -2.303 x 8.314 x 365 log K log K = 2.36 = log ( 2.30…

Q: The following reaction has an Eo value of -0.76 V: H2(g) + Zn2+(aq)----->Zn(s) + 2H+(aq) a.…

A: You have given - Eocell = -0.76 V temp = 298 K

Q: At 355 K, ∆G = -5.7 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are…

A: The given reaction is A (g) → 2 B (g) Partial pressure of A = p(A) = 7.05 atm Partial pressure of B…

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

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Q: For the reaction I2(g) + Cl2(g)2ICI(g) AH° = -26.8 kJ and AS° = 11.4 J/K The equilibrium constant…

A: In this question, we have to calculate the equilibrium constant for the given reaction with the…

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

A: From thermodynamics data we can calculate equlirbrum constant for a reaction with the help of…

Q: At 298 K. AG°=+20.9 kJ/mol for the reaction CH;CO,H (aq) =H (aq) + CH;CO2 Calculate AG for this…

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Q: For a particular reaction, AH = 120.5 kJ and AS = 758.2 J/K. Calculate AG for this reaction at 298…

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Q: For a particular reaction at 199.1 °C, AG = -159.63 kJ, and AS = 894.41 J/K. Calculate AG for this…

A: Given data for a particular reaction at temperature 199.1°C ,  T = 199.1°C = (199.1+ 273) K = 472.1…

Q: At 355 K, ∆G = -1.3 kJ/mol for the reaction A (g) → 2 B (g). If the partial pressures of A and B are…

A: The pressure of individual gas when kept alone is known as partial pressure of that gas.

Q: Hemoglobin, abbreviated Hgb, reacts with a certain oxide, XO, and oxygen gas, 02. Consider the…

A: The overall reaction of displacement of oxygenated hemoglobin with other oxides takes place as…

Q: Predict the sign of entropy change for the following reaction. Ag+(aq) + Cl-(aq) – AgCI(s)

A: Entropy is defined as a measure of randomness or disorder of a system. More the randomness, more is…

Q: Using the thermodynamic information, calculate the standard reaction free energy for the reaction…

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Q: The standard free energy of formation of ammonia at 298 K is -16.5 kJ/mol. a) Calculate AG for the…

A: Given,  Standard Gibb's free energy of formation= ΔGf0 = -16.5 KJ/mole  Reaction is :  N2 (g) + 3H2…

Q: The thermodynamic values from part A will be useful as you work through part B:   ΔH∘rxn…

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Q: Explain how a reaction that is not spontaneous may be driven forward by coupling it to a spontaneous…

A: A reaction that is capable of carrying a reaction in forward direction without any use of external…

Q: 1. a. Calculate AG° at 298 K for the reaction: Cu2S(s) + O2(g) → 2Cu(s) + SO2(g) K = 3.25 x 1037 b.…

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Q: A student determines the value of the equilibrium constant to be 1.98×107 for the following…

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Q: For the reaction NH,CI(aq)NH3(g) + HCI(aq) AH° = 86.4 kJ and AS° = 79.1 J/K The equilibrium constant…

A: The reaction given is, => NH4C (aq) --------> NH3 (g) + HCl (aq) Given : ΔHo = 86.4 KJ = 86400…

Q: Predict the following reaction, whether its spontaneous or nonspontaneous. a. 2NAOH) + CO2s) b. 2Fe…

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Q: The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn…

A: We have given that ∆G° = 1.92×105 J/mole T  = 298 K ∆H° = 243.5 kJ /mole ∆S° = 170 J/mole = 0.170…

Q: Given the information AS' = 302.0 J/K AS“ = -153.0 J/K A + B → 2D AH' = 699.7 kJ C- D AH' = 398.0 kJ…

A: In this question, we first have to find out the values by using Gibbs free equation, ∆G°=∆H°-T∆S°…

Q: For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic…

A: The thermodynamic relation that will be used here is as follows: ∆G°=∆H°-T∆S°     ... (1) where ∆G°…

Q: Given the information A+ B 2D AH = 754.9 kJ AS" = 326.0 J/K %3D C- D AH = 427.0 kJ AS = -236.0 J/K…

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