Calculate the value of ΔdissolveG0 from the values of ΔdissolveH0 and ΔdissolveS0 and comment on the spontaneity of the dissolution process.   ΔoplosG0/kJ mol-1 = ΔoplosH0-TΔoplosS0 = 19.69 kJ mol-1 - (298.15 K) x (80.15 x 10-3 kJ K-1 mol-1) = -4.21 kJ m

Q: Determine the ΔSsurr when 9.01 g of steam→ liquid at 100 ̊C (ΔHvap = 40.67 kJ/mol, ΔSsurr = -q/T)

A: First, we need to convert the mass of steam to moles. The molar mass of water (H2O) is approximately…

Q: 5.The following describes the process occurring spontaneously if the system is a hotter object…

A: 5) Given : System is a hotter object. Since the system is a hotter object. Hence the temperature of…

Q: a) Calculate the Gibbs energy change for the following reaction at 27.00°C. Answer with four…

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Q: Suppose 50.0 g of superheated Na(s) melts at 500 K and 1 bar pressure. Find the ΔSsys, ΔSsurr​, and…

A: Melting of Na is a reversible change. So,  ∆Ssys=∆qT and,∆Ssurr =-∆qTHere, ∆q= m×Cp×∆Tm= mass. Cp=…

Q: The literature value for the solubility of borax at 25oC is 1.2 X 10-2.  Predict the Ksp at 25oC…

A: Given: ∆S°=590 J/mol.K ∆H°=188.69 kJ/mol The literature value for the solubility of borax at 25oC =…

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

A: Given that: ∆Go=-32.8 KJ/mol T = 298 K PN2=0.200 atm PH2 = 0.400 atm PNH3 = 0.900 atm To find, ∆G…

Q: he free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: For the dissociation of borax reaction, standard enthalpy change, ∆Ho = 188.69 kJ/mol standard…

Q: Using data from enthalpies and free energy of standard formation that we attach below, a) determine…

A: (a) The standard thermodynamic data for the given reactants and products at given temperature is,…

Q: Data: Room Temperature of Borax = 23˚C Kₛₚ of borax at room temperature trials First: 21 mL of HCl…

A: The balanced equation for the dissociation of borax, Na2B4O5OH4.8H2Os is: Na2B4O5OH4.8H2Os⇌2Na+aq +…

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

A: Formula used:-  ∆G = ∆G° + RT ln Kp Where Kp is pressure of product/pressure of reactant

Q: For a certain chemical reaction, the equilibrium constant K Round your answer to 2 significant…

A: The standard Gibbs free energy change (ΔG°) and the equilibrium constant (K) are related by the…

Q: What is the standard change in Gibbs free energy of this reaction at 25 °C?

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Q: For each reaction, calculate AHn, ASn , and AGn at 25 °C and state whether or not rxn rxn the…

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

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Q: Calculate the temperature at which Δ G system = 0 ifΔ H system = 4.88 kJ and Δ S system = 55.2 J/K.

A: Given data : Δ G system = 0 Δ H system = 4.88 kJ  Δ S system = 55.2 J/K We have to calculate the…

Q: 0,- M,0,0) 2 M(s) + r this reaction, AHn = -5.268 kJ/mol and A.S = 10.78 J/(mol-K) at 298 K. hat is…

A: The question is based on the concept of equilibrium. we have to calculate Gibbs free energy &…

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: Chemistry  (i) For T = 298K ΔG° = -8.314 x 298 x ln (2.83x10-3) = 14.524 KJ/mol (ii) For T =…

A: The thermodynamic equation for Gibbs free energy is,∆G=∆H-T∆SFrom the graph of ∆G vs T, Comparing…

Q: For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH = -81.1 kJ and AS = -1.20 J/K The…

A: The objective of the question is to calculateThe equilibrium constant for the reaction at .The…

Q: What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M…

A: The balanced chemical equation is: 2NO(g) + O2(g) → 2NO2(g)   Temperature, T = 298.15 K which is the…

Q: Combustion of glucose (C6H12O6) is the main source of energy for animal cells: CHO) +60, (e) 600,…

A: (0.00855501 g of glucose)Rounded to two significant figures0.0086 g  of glucoseExplanation:Given the…

Q: the free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: When solid borax is added to water, the following equilibrium is established.…

Q: X After 2.00 × 10² g of gold (Cp,s = 0.131 J g-¹ K-¹) at 120.0 °C is dropped into 25.0 g of water…

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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: Ca2"(ag) + 2 F(aq) O 37.3 kJ mor he following standard enthalpy and entropy of reaction: IkJ mor…

A: Change in gibbs free energy of a process can be calculated as :

Q: What is the standard heat of reaction for the given equation? What is the standard entropy for the…

A: Here we are required to find the Gibbs energy for the given reaction at the specified temperature…

Q: For a chemical reaction the equilibrium constant was found to be K = 1.4 × 10–8 at T = 298.15 K, and…

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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: 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: Thermodynamic data were collected for a reaction where sodium chloride was dissolved in water at…

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Q: the free energy for a reaction can be related to the equilibrium constant through the formula below.…

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Q: A box contains a gas composed of 12 atoms each corresponding to the different stable isotopes of Tin…

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Q: In glycolysis, the hydrolysis of ATP to ADP is used to drive the phosphorylation of glucose (GLC):…

A: In glycolysis, the hydrolysis of ATP to ADP is used to drive the phosphorylation of glucose (GLC):…

Q: AG OAS > 0 for this process. ΔΗ = TAS at a certain temperature. AH° > 0 for this process. The…

A: For Gibbs free energy we have equation : ∆G° = ∆H° - T∆S° So, above graph is a straight line…

Q: the free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: Given: When solid borax is added to water, the following equilibrium is…

Q: of 16 For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: The given equilibrium reaction is N₂(g) + 3 H₂(g) 2NH3(g)The standard change in Gibbs free energy…

Q: 4NH3+6NO=>5N2+6H2O , Find the molar heat of reaction ΔH, For the reaction at 298K. Give your answer…

A: Given: Temperature (T1) = 298 K Temperature (T2) = 335 K

Q: The equilibrium constant for a certain reaction increases by a factor of 6.48 when the temperature…

A: Relationship between two equilibrium constant at two different temperatures is ln ( ) = Where K1 is…

Q: Consider the reaction A  -> 2 B. Suppose 2.50 mol of A is initially introduced into a 1.00 L flask.…

A: Given data: Moles of A=2.50 mol. Volume=1.00 L. Temperature T=25°C=298 K. The concentration of B is…

Q: The decomposition reaction, C(g) A(g) + 2B(g) has Kc = 41 at 298 K. What is the value of K, for this…

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Q: Mixture ΔT NaCl + H2O -0.2  NaNO3 + H2O -0.9 NaCH3COO + H2O 0.9   Which reactions are endothermic?…

A: For any reaction process, if the temperature goes on decreasing, this means heat has been evolved…

Q: 17. For which of the following highly exothermic processes would you expect AH" and AG to be about…

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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: Under which conditions is a reaction non-spontaneous at all temperatures, according to AG = AH – TAS…

A: In this question we have to tell the condition for non spontaneous at all the temperature.

Q: The following reaction presents a ΔH0 and ΔG0 of 217.9 kJ/mol and 72.4 kJ/mol respectively, at 600…

A: ReactionCH4 (g) + H2O (g) → CO(g) + 3H2 (g)∆H° = 217.9 kJ /mol∆G° = 72.4 kJ/molTemperature = T = 600…

Q: 50.0 mL of 1.0 M HCl (at 22.0ºC) and 50.0 mL of 1.5 M NaOH (at 22.0ºC) are mixed. The solution…

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