For the reaction 2BRF3(g) Br2(g) + 3F2(g) AH° = 542 kJ and AS° = 269 J/K %3D AG° would be negative at temperatures (above, below) K.

Q: 19.65 A particular constant-pressure reaction is barely sponta- neous at 320 K. The enthalpy change…

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Q: Consider the reaction at 298 K. 2 C(graphite) + O2(g) 2 CO(g) AH° = -221.0 kJ/mol > Calculate the…

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Q: For the reaction N2(g) + 3H2(g) = 2NH3(g), Kp = 1.60 × 104 at 400°C. Calculate a) AG°n b) AGrxn when…

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Q: Fe(s) + 2HCI(aq)→FeCl2(s) + H2(g) for which AH° = -7.400 kJ and AS° = 107.9 J/K at 298.15 K. (1)…

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Q: Use the References to access important values if needed for this question. Without doing any…

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Q: What is the standard Gibbs free energy of the reaction H2(g) + Br2(g) → 2HB1(g) at 298 K, and is it…

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Q: Given the information A+B C 2D D calculate AG at 298 K for the reaction A+B 2C AG = - AH = -742.7 kJ…

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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: a Use data given below to obtain the value of K, at 1500.°C for the reaction C(graphite) + CO2(9g) =…

A: It is given that graphite is combining with carbon dioxide to produce carbon monoxide and the…

Q: For the reaction 4NH3(g) + 50,(g)–→4NO(g) + 6H,O(g) AH° = -905.2 kJ and AS° = 180.5 J/K The standard…

A: Change in standard free energy calculation:

Q: Calculate the value of delta G at 225 °C and 1 atm for the reaction below,   2O3 +3I2 => 6IO…

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Q: If E°cell > 0, then what the value is of change in Gibbs free energy (G and the process is…

A: Given:: E°cell> 0 ∆G° = ?

Q: Consider the following reactions. (a) C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4H₂O(g) AH rxn = -2044 kJ…

A: we need to consider the Gibbs free energy change (ΔG) for each reaction. The Gibbs free energy…

Q: If AS at 25°C sys =-198.3 J/K, is the reaction spontaneous N2 + 3H2 → 2NH3 • AS univ = AS sys + AS…

A: The enthalpy change of the reaction (ΔH reaction) can be calculated using the…

Q: Calculate the change in the Gibbs energy for the reaction below, at 25.0 °C 2 Ca(s) + O2(g) → 2…

A: The formula for Gibbs free energy change is written as - ∆G° = ∆H° - T∆S°   Where - ∆G° = Gibbs free…

Q: For the reaction N2(g) + 3 H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the…

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

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

A: Information of question

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: ΔΗ 92. kW J AS = 164. K - 2NH, (2) ) – N, (e) + 3H, (g) AG = Which is spontaneous? O this reaction…

A: ∆G=∆H-T∆S      at 25°C For reaction to be spontaneous, ∆G<0 And for reaction to be…

Q: For the reaction NH,NO3(aq) → N½O(g) + 2 H,0(1) AG° =-177.8 kJ and AH° = -149.6 kJ at 282 K and 1…

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Q: Consider the reaction 2NO(g) + O₂(g)→→→→→2NO₂(g) Using the standard thermodynamic data in the tables…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: For the reaction CACO3(s)- → CaO(s) + CO2(g) AG° = 137.0 kJ and AH = 178.3 kJ at 257 K and 1 atm.…

A: In this question, first we will Identify it is reactant favored or Product favored.  Then we will…

Q: Consider the reaction SO₂(g) + 2C(s,graphite)—S(s,rhombic) + 2CO(g) for which AH° = 75.80 kJ and AS°…

A: Consider the reactionSO2(g) + 2C(s, graphite) →S(s, rhombic) +2CO(g)for which ∆H° = 75.80 kJ and ∆S°…

Q: C,H (g) – H,(g) + C,H,(g) Use the data from the table below and use the formula : AG° = AH°-TĀS°…

A: Here, we have to calculate the value of ∆G° at 298 K Temperature, T = 298 K

Q: For a process with AH 0 O AS > 0 ΟΔΕ>0 O Never.

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Q: At 298 K, this reaction to produce phosphoryl chloride has a standard enthalpy of A,H° = -620.2 kJ…

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Q: Given the information A+B 2D CID calculate AG" at 298 K for the reaction AG' AH' = 792.8 kJ AH' =…

A: Given data:

Q: 6) Calculate AH98 for the processe 5 Sb(s) + CI, (8) → SBCI, (g) from the following information:…

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Q: or the reaction H₂Cl(aq)- NH3(g)+ HCl(aq) H° 86.4 kJ and AS° = 79.1 J/K the equilibrium constant for…

A: The reaction given is,NH4Cl (aq) --------> NH3 (g) + HCl (aq)Given : ΔHo = 86.4 KJ = 86400 J…

Q: For the reaction 2H₂O(1)→ 2H₂(g) + O2(g) AG = 472 kJ and AH = 572 kJ at 306 K and 1 atm. This…

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Q: Describe the spontaneity of the following reactions. ΔΗ=91.8 W 1. Nye + 3H ---→ 2NH3 ΔΗ= 29.1 kJ 2.…

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Q: Consider the reaction 2NaOH(aq) + H₂(g) 2Na(s) + 2H₂O(l) for which AH° = 368.6 kJ and AS° = 15.30…

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Q: al ula O [The reaction 2H,O(g) 2H2(g) + O2(g) is expected to have a positive value of AS°.] O [If a…

A: Entropy is defined as the degree of randomness or disorderliness of the System.   if the molecules…

Q: For the reactionP4O10(s) + 6H2O(l ) ----> 4H3PO4(aq)ΔG° = -447.8 kJ and ΔS° = -16.3 J/K at 329 K…

A: ΔG on reaction of 1.00 mol P4O10 is -447.8 kJ. Hence, ΔG on reaction of 1.80 mol P4O10 is 806.0 kJ…

Q: Consider the reaction Ca(OH)₂(aq) + 2HCl(aq)→→CaCl₂(s) + 2H₂O(1) for which AH° = -30.20 kJ and AS° =…

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Q: Calculate the AG for the vaporisation of mercury at 24°C using AH = 61.0 kJ mol-1 and AS = 89.0 J…

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Q: (a) 1 Sn+ (aq) + 1 Hg(l)--> 1 Sn²+ (aq) + 1 Hg2+ (aq) (b) 2 Hg²+ (aq) + 1 Co(s) --> 1 Hg₂²+ (aq) + 1…

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Q: If AS at 25°C sys =-198.3 J/K, is the reaction spontaneous N2 + 3H2 → 2NH3 • AS univ = AS sys + AS…

A: The enthalpy change of the reaction (ΔH reaction) can be calculated using the…

Q: For the reaction Fe,O3(8) + 3H2(g)-2Fe(s) + 3H2O(g) AH° =98.8 kJ and AS° 142.5 J/K The equilibrium…

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Q: 21. Predict whether the equilibrium for the photosynthesis reaction described by the equation 6…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

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.