Determine the temperature of a reaction if K = 1.20 x 10-6 when AG° = +39.40 kJ/mol.

Q: For the reaction Ca(OH)2(aq) + 2HCl(aq)CaCl2(s) + 2H2O(l) H° = -30.2 kJ and S° = 205.9 J/K The…

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Q: Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0…

A: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical…

Q: Determine AG° for the reaction N2O4(g) = 2 NO2(g) (K= 0.144 at 298 K).

A: Given :- K = 0.144                T = 298 K  To be calculated :- ∆G° (in kJ/mol)    Formula :- ∆G° =…

Q: A certain reaction has an equilibrium constant of 10.1 at 25oC. Determine the ΔGo in kJ/mol

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Q: Determine K for a reaction at 200 K if AG° =24.6 kJ/mol. (R = 8.314 J/mol · K)

A: Given  Temperature ( T ) = 200K  Standard Gibbs free energy ( ∆G° ) =  24.6 KJ/mol…

Q: The equilibrium constant for the reaction               2Fe3+(aq) + Hg22+(aq) ⇌ 2Fe2+(aq) +…

A: The standard Gibbs free energy and equilibrium constant are linked by the expression ΔG°=-RTlnKC…

Q: For the reactionA(aq) ---> B(aq) the change in the standard free enthalpy is 3.23 kJ at 25 oC and…

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Q: Which of the folowing statements about the standard Gibbs energy change for the reaction, 4,G° is…

A: Given: To find the best statement related to ΔrGo for the reaction.

Q: Determine K for a reaction at 200 K if AG° =22.7 kJ/mol. (R = 8.314 J/ mol · K)

A: Can find answer in the image below

Q: Determine K for a reaction at 200 K if AG° =22.8 kJ/mol. (R = 8.314 J/mol · K)

A: Given is ΔG° = 22.8 kJ/mol = 22800 J/mol T = 298 K R = 8.314 J/mol-K We are to find the equilibrium…

Q: For the reaction N2(g) + O2(g)2NO(g) AH° = 180.6 kJ and AS° = 24.9 J/K The equilibrium constant for…

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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: Determine K for a reaction at 200 K if ∆G° =11.6 kJ/mol. (R = 8.314 J/mol ･ K)

A: The relation between the standard Gibbs free energy change and the equilibrium constant is as…

Q: For a particular reaction at 222.1 °C, AG =-848.94 kJ, and AS = 171.81 J/K. Calculate AG for this…

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Q: Determine the equilibrium constant K for the following reaction at 298 K. Cl(g) + O3(g) - CIO(g) +…

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Q: Determine K for a reaction at 200 K if AG° =15.1 kJ/mol. (R = 8.314 J/mol · K)

A: Given :-  ∆G° = 15.1 kJ/mol  R = 8.314 J/mol.K  T = 200 K  To determine :-  Value of K

Q: Determine the equilibrium constant for the following reaction at 298 K.               SO3(g) +…

A: Given reaction:

Q: For the reaction NH4Cl(aq) NH3(g) + HCl(aq) AH° = 86.4 kJ and AS° = 79.1 J/K The equilibrium…

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Q: Calculate Kp for the reaction 2NOCI(g) –> 2NO(g) + Cl2(g) at 400C if Kc at 400C f- = reaction is 2.1…

A: We will use relation between kp and Kc.

Q: Determine the equilibrium constant for a reaction at 260.0 K if ∆G° =21.20 kJ/mol. (R = 8.314 J/mol…

A: Given: Temperature is 260 K ∆G° is 21.20 kJ/mol Gas constant, R is 8.314 J/mol. K To find:…

Q: The equilibrium constant for a reaction is 0.48 at 25 °C. What is the value of ΔG° (kJ/mol) at this…

A: the relationship between gives free energy and equilibrium constant is given as  ∆G°= -RTlnK  where…

Q: Determine the temperature of a reaction if K = 1.2 x 10-6 when AG° = +20.6 kJ/mol.

A: Given: ΔGo=+20.6 kJ/mol=+20.6 x 103 J/mol K=1.2 x 10-6  Temperature, T=?

Q: The equilibrium constant, Kc, for the following reaction is 6.50x10-3 at 298 K. Calculate K, for…

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Q: The oxidation of nitrogen monoxide is favored at 457 K 2NO(g)+O₂(g)⇌ 2NO₂(g) Kₚ=1.3X10⁴ (a)…

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Q: How does the value of ΔG° for a reaction relate to the equilibrium constant for the reaction?

A: The relation between ΔG° for a reaction and the equilibrium constant is given by,

Q: Calculate the equilibrium constant for the reaction from the following thermodynamic data, when the…

A: Thermodynamics is the branch of chemistry that deals with the study of heat and other forms of…

Q: For the reaction CaO(s) + CO2(g) CACO (s) %3D 4.1 X 103 ΔΗΟ -42,500 – 0.66 T + 2.155 X 10-3 T² + T…

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Q: Consider the following reaction at 298 K. Co2+ (aq) + 2Ag(s) → Co(s) + 2Ag+ (aq) Which of the…

A: Given reactions: Co2+(aq) + 2Ag(s) → Co(s) + 2Ag+(aq) Hg2+(aq) + Cd(s) → Hg(l) + Cd2+(aq) We have to…

Q: 6) Determine the equilibrium constant for the following reaction at 298 K. SO3(g) + H20(g) –…

A: SO3(g) + H2O(g) ------> H2SO4(l) Given, Temperature = 298 K ∆G° = -90.5kJ Formula, ∆G = ∆G° +…

Q: Determine the temperature of a reaction if K = 1.20 x 10-6 when AG° = +24.10 kJ/mol.

A: Gibbs free energy is the maximum amount of non-expansion work that can be drawn from a system. Gibbs…

Q: When a AH>0 and TAS<0 the reaction will be: а. spontaneous O b. system is an equilibrium С. not…

A: The reaction will be not spontaneous if  Delta G &gt; 0  And in this question we have to tell that…

Q: Determine K for a reaction at 200 K if ∆G° =16.7 kJ/mol. (R = 8.314 J/mol ･ K)

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Q: How does the value of ∆G° for a reaction relate to the equilib-rium constant for the reaction? What…

A: Relationship between standard Free energy ∆G° and the equilibrium constant is as follows: ∆G = ∆G°…

Q: For the reaction N2(g) + 20,(g)→2NO,(g) AH° = 66.4 kJ and AS° =-121.6 J/K The equilibrium constant…

A: The reaction given is, =&gt; N2 (g) + 2 O2 (g) --------&gt; 2 NO2 (g) Given : ΔHo = 66.4 KJ = 66400…

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: Determine the temperature of a reaction if K = 1.20 x 10-6 when AG° = +22.70 kJ/mol. %3D

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Q: For the reaction NH4NO3(aq)N2O(g) + 2H2O(l) H° = -149.6 kJ and S° = 99.9 J/K The equilibrium…

A: Spontaneous processes are those processes which take place on their own without providing any energy…

Q: 10. Determine the equilibrium constant for the following reaction at 298 K. SO3 (g) + H2O (g) →…

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Q: Determine the K, for CN at 25°C. The K for HCN is 4.9 x 10 10 O 2.3 x 10-9

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Q: For the reaction N2(g) + 3H2(g)–→2NH3(g) AH° = -92.2 kJ and AS° =-198.7 J/K The equilibrium constant…

A: When rate of forward reaction become equal to rate of backward reaction, then a reversible reaction…

Q: For the reaction CO(g) + 3H2(g)–→CH¼(g)+ H20(g) AH° = -206.1 kJ and AS° = -214.7 J/K The equilibrium…

A: The question is based on the concept of chemical equilibrium. We have to calculate the equilibrium…

Q: Consider the reaction at 25°C, where CACO3(s) decomposes to form CO2(g) + CaO(s) If the standard…

A: Given  Standard Enthalpy Change ( ∆ H0 ) = 179.2 KJ  Temperature ( T ) =25 ℃…

Q: Which of the following statements about the standard Gibbs energy change for the reaction, A,G° is…

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Q: what is ΔG for a certain reaction of 300 degrees Kelvin if Kp is 6.0 x 10^2

A: Given-&gt; T = 300 K Kp = 6.0 × 102

Q: Determine the temperature of a reaction if K = 1.20 x 10-6 when AG° = +22.70 kJ/mol.

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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, =&gt; NH4C (aq) --------&gt; NH3 (g) + HCl (aq) Given : ΔHo = 86.4 KJ = 86400…

Q: For the reaction NH4NO3(aq)N2O(g) + 2H2O(l) H° = -149.6 kJ and S° = 99.9 J/K The equilibrium…

A: The relationship between the change in free energy (∆G°), change in enthalpy (∆H°) is furnished as…

Q: Determine the equilibrium constant, Keq, at 25oC for the reaction: Au3+(aq) + Al(s)   →   Au(s) +…

A: The reaction given is  Au3+(aq) + Al(s)   →   Au(s) + Al3+(aq)

Q: The equilibrium constant, K, for the following reaction is 6.50×10 3 at 298 K. Calculate Kp for this…

A: We have find out Kp for reaction.

Q: Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0…

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.