Calculate ΔG^0 (in kJ/mol) given ΔG= -726.6 kJ/mol and R= 0.008314 kJ/mol K and T= 824.5 K and Q=0.554 ΔG=ΔG^0+RTlnQ answer choices: a) -733 b) -240 c) -725 d) -723 e) -727

Q: ΔG

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Q: What is AH°, for the following phase change? Q (1) → Q (s)

A: Enthalpy change for this phase transition is determined as :

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: S° (J/molK) S° AHL (kJ/mol AGE (kJ/mol) AG? (kJ/mol (kJ/mol) | (J/molK) AHE Substance Substance

A: The missing thermodynamic parameter value is to be provided.

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 -…

Q: At what temperature (K) does a reaction becomes spontaneous when ΔS = -382 J/mol-K and ΔH = -182.7…

A: ΔG = ΔH - TΔS For a reaction to be spontaneous: ΔG = -ve

Q: 2NO(g)+O2(g)→2NO2(g)ΔH°=−112kJ/molrxn Answer the following questions about the reaction represented…

A: Please have a look on the sol:

Q: C₂H₂(g) +30₂(g) →→→→2CO₂(g) + 2H₂O(g) C₂H4(8) O2(g) CO₂(g) H₂O(g) AH°f, kJ/mol 52.3 0 -393.5 -241.8…

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Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 4.0 at 295 K? (R = 8.314 J/mol ･ K)

A: The given problem can be solved by using the formula given below as; ∆G = ∆G° + 2.303 RT log Q…

Q: Calculate the temperature at which Δ G system = -34.7 kJif Δ H system = -28.8 kJ and Δ S system =…

A: Formula : Δ G system = Δ H system - TΔ S system  -34700 J = -28800 J - T x 22.2 J/K - 22.2 T =…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 3.0 at 295 K? (R = 8.314 J/mol ･ K)

A: The spontaneity and feasibility of reaction can be predicted by the Gibb’s free energy of that…

Q: Calculate ΔEΔE, if q=q= 0.768 kJkJ and w=w= -880 JJ

A: We have given that q = 0.768KJ W = -880J = -0.880KJ ∆E = ?  So According to first law of…

Q: a) What is K for a reaction if ∆G° =151.6 kJ/mol at 25.0 °C? (R = 8.314 J/mol ･ K) b) For the…

A: We know- ΔG = ΔG° + RT ln QandΔGo=-RTlnK now we have to rearrange the equation- ΔG = ΔG° + RT ln QΔG…

Q: Calculate ΔG^0 (in kJ/mol) given ΔG= -833.7 kJ/mol and R= 0.008314 kJ/mol K and T= 261.5 K and…

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Q: Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15…

A: As well as increases the negative value of standard free energy . The reaction is spontaneous in…

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: Which reaction is spontaneous at SATP? AH=41.5 kJ, AS=-12.9 J/K AH=8.75 kJ, AS=21.2 J/K AH=24.9 kJ,…

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Q: Use the AH° and AH xn information provided to calculate AH°, for IF: IF7(g) IF5(g) AH°F (kJ/mol)…

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Q: Given the information A+B 2D C D ΔΗ° = 739.8 ΚΙ AH° = 453.0 kJ AS 314.0 J/K AS-167.0 J/K calculate…

A: The objective of the question is to calculate the Gibbs free energy change (ΔG°) for the reaction…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 0.14 at 295 K? (R = 8.314 J/mol ･ K)

A: Given: ∆G° = -4.5 kJ/mol Q = 0.14 Temperature = 295 K R = 8.314 J/mol ･ K

Q: Calculate ΔG0 (in kJ/mol) given ΔG= -423.1 kJ/mol and R= 0.008314 kJ/mol K and T= 611.3 K and…

A: Given: ΔG= -423.1 kJ/mol R= 0.008314 kJ/mol K  T= 611.3 K  Q=0.601Required: ΔG0 (in kJ/mol) = ?…

Q: Calculate ΔΔS° for the evaporation of water, given S°[H2O(l)] = +69.9 J/mol.K and S°[H2O(g)] =…

A: During evaporation, the liquid water converts into water vapour. In this process, the entropy of the…

Q: ΔS of N2 = 191.6 J/mole⋅K ΔS of H2 = 130.6 J/mole⋅K ΔS of NH3 = 192.7 J/mole⋅K   Calculate the…

A:

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: Le Chatelier's Principle: Calculate ΔH if K doubles when T increases from 298 K to 308 K. (answer =…

A: The Arrhenius equation is: logK2 K1=Ea2.303R1 T1-1 T2 Here K is the rate constant. Ea is the…

Q: Calculate ΔGo at 91oC for the dissolution an ionic solid which has a Ksp of 2.2 x 10-8 at 91oC.…

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Q: P4(s)+5O2(g)⟶P4O10(s)                                ΔG°=−2697.0 kJ/mol 2H2(g)+O2(g)⟶2H2O(g)…

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Q: Given the information A+B 2D AH = 641.6 kJ AS 335.0 J/K C D AH* = 488.0 kJ AS-146.0 J/K calculate AG…

A:

Q: Calculate ΔG0reaction in kJ/mol at 298.15 K given Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)…

A:

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: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 0.54 at 295 K? (R = 8.314 J/mol ･ K)

A:

Q: What is ∆G° for the reaction I₂(g) → 2 I(g) at 25.0 °C if K = 6.1 x 10⁻²²? (R = 8.314 J/mol･K)

A: We are authorised to solve only one question at a time. Please post rest of the questions…

Q: In a typical cold pack (used for sports injuries), a salt such as ammonium nitrate is kept in a…

A: Dissolution of ammonium nitrate in water is given by, NH4NO3(s)→H2O(l) NH4+(aq)+NO3-(aq)   ∆H=+25.09…

Q: 16. Use the thermochemical data that follow to calculate the value of AHⓇ for the reaction: 4 B 2A +…

A:

Q: Calculate the Ksp for the dissociation of solid barium nitrate in water at 25.0 oC.  The ΔGo for…

A: given -  ΔGo for Ba(NO3)2(s) = -797 kJ/mole. temperature T = 25.0 oC. = 25+ 273 = 298 K Ksp = ?

Q: Comment on whether ΔH and ΔS favor spontaneity of the following reactions. Explain your reasoning!…

A: Spontaneous reaction are those which occur in forward direction and favour the formation of product.

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 2.5 at 295 K? (R = 8.314 J/mol ･ K)

A: According to thermodynamics equation, dG = dG° + RTlnQ On solving above equation we get,

Q: Determine ΔG0 at 298 K for N2(g) + 3 H2(g) <---> 2NH3(g) given Substance ΔH0f (kJ/mol)…

A: The given reaction is, N2(g) + 3H2(g) → 2NH3(g) The enthalpy change of the reaction can be…

Q: Calculate ΔS^0reaction in J/mol at 298.15 K given N2(g)+O2(g)→2NO(g)…

A:

Q: Calculate T (in K) given ΔG0= -35.7 kJ/mol and ΔH0= 39.7 kJ/mol and ΔS0= 404 J/mol K ΔG0=ΔH0−TΔS0

A: ΔG° = -35.7 kJ/mol ΔH° = 39.7 kJ/mol and ΔS° = 404 J/mol K We use  following formula to calculate…

Q: N2(8) + 3F2(g) → 2NF3(g) N2(g) + 3C12(g) → 2NC13(g) AH° = 460 kJ AS® = -275 J/K N2F4(g) → 2NF2(g)…

A: Since you have posted question with multiple subparts as per guidelines we can answer only three per…

Q: Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) +…

A: Given that ,  Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ;  ΔH°1= -452kJ MgO(s) + 2HCl(aq) → MgCl2(aq) +…

Q: 15) Calculate the AG°₁ AHᵒf (kJ/mol) S°(J/mol K A) +50.8 kJ rxn at 298 K using the following…

A:

Q: 2N205 (g) → 4NO2 (g) + 02 (g) at 25°C, for which the following data are relevant: AH°, (kJ/mol) S°…

A: For a reaction  2N2O5 (g) ——> 4 NO2 (g) + O2(g) delta H of formation  delta S and temperature is…

Q: Use the following deltaG degrees f values to calculate deltaG degreesrxn for the following reaction.…

A: Use the following deltaG degrees f values to calculate deltaG degreesrxn for the following reaction.…

Q: 160.95 205.0 O(g) 02(g) FeO(s) Fe203(s) FegO4(s) Fe(OH)2(s) 60.8 90.0 145.2 79.5 che answer should…

A: As we know, for a chemical reaction,  □Srxn = [Total entropy of products] - [Total entropy of…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 1.6 at 295 K? (R = 8.314 J/mol ･ K)

A: Given: Standard Gibbs free energy change, ∆G° = -4.5 kJ/mol Reaction quotient, Q = 1.6 Temperature,…

Q: CHEMWORK Use the values of S° given below to calculate AS° for the following reaction: 2Na(s) +…

A: Calculate change the entropy of the given above reaction --