The Eᵒcell and the reaction are given below. What is the Gibbs free energy of the system at standard conditions? Pb²+ (aq) + Mg(s) = Pb(s) + Mg2+ (aq) Ecell = +2.24 V Eº AG° = [?] kJ
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![The Eᵒcell and the reaction are given
below. What is the Gibbs free energy of
the system at standard conditions?
Pb²+ (aq) + Mg(s) = Pb(s) + Mg²+ (aq)
Ecell = +2.24 V
AG° = [?] kJ
Enter either a + or - sign AND the magnitude in
your answer.
Free Energy, kJ
Enter](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe00a13c6-9542-4fe0-b265-b511cc58972b%2F2aa475db-3344-4aa5-b75a-4c55a80585fd%2F1ozkmx_processed.jpeg&w=3840&q=75)
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- The standard Gibbs free energy change is 2.60 kJ/mol for the reaction at 25.0oC: H2(g) + I2(g) →← 2HI(g); ∆Gorxn = + 2.60 kJ/mol The reaction starts with equal molar amounts of H2(g) and I2(g) in a previously evacuated, constant volume vessel. What is the equilibrium mole fraction of HI? Enter your answers with correct units and significant figures.of 16 For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) = 2NH₂(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH, = 0.750 atm? AG = kJ/mol.For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g)N2(g) the standard change in Gibbs free energy is Δ?°=−69.0 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?N2=0.250 atm, ?H2=0.150 atm, and ?NH3=0.600 atm?
- Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 24.4 at 25oC and 35.7 at 50oC. What is the value of the standard Gibbs free energy change (in kJ) of this reaction at 75oC?The value of the equilibrium constant at 25ºC, corresponding to the reaction: 3 C2H2 (g) = C6H6 (g), is Keq = 1.22 Taking into account this information, indicate V or F as appropriate,Justify:I) The Gibbs free energy of this reaction is = 0II) The Gibbs free energy of this reaction is <0III) The reaction is spontaneous to the rightIV) It is advisable to manufacture benzene under these conditions.a) TFTF b) TTTT c) FFTT d) FTTT e) FTFT f) TFTT g) TFFF
- 2. Calculate the ∆G (non-standard) in kJ for the following reaction at the given pressures and 25°C: 2H2 (g) + O2 (g) --> 2H2O (g) PH2= 0.775 bar PO2= 2.88 bar PH2O= 0.556 bar ∆G° under standard conditions= -457.14 kJA student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = JCalculate the equilibrium constants Keqo for the following reactions, using the standard free energy changes given below. (Note: if your calculation produces an overflow error, give the answer as a power of e.)a) Glucose + 6O2 --> 6CO2 + 6H2O (–2,840 kJ/mol)b) ATP + H2O --> ADP + Pi (–30.5 kJ/mol)c) Ethyl Acetate + H2O --> Ethanol + Acetate (+19.6 kJ/mol)
- standard change in the gibbs free energy of the molar reaction is -2315kj what is the difference between the reduction reaction’s electric potential and oxidation reaction.Given the following chemical reaction and standard thermodynamic quantities in the table, Cu(s) + H2O(g) ⟶ CuO(s) + H2(g) Cu(s) H2O(g) CuO(s) H2(g) ∆H°f (kJ/mol) 0 −241.8 −155.2 0 ∆S° (J/mol∙K) 33.3 188.7 43.5 130.6 at 500 K, ∆G° for this reaction is [ Select ] ["86.74 kJ", "231.8 kJ", "‒58.6 kJ", "110.6 kJ"] , and the reaction is [ Select ] ["spontaneous at this temperature", "nonspontaneous at this temperature"] .H2O(S) = H2O(L) We already know that the Gibbs energy change of the reaction is 0 J/mol reaction at 0 oC and 1 bar. Calculate the Gibbs energy change of the reaction at 1.18 oC and 1 bar. ΔrG = _________ J/mol. 3 sig. fig. The following data are copied from the appendix of the textbook and assuming constants in the temperature region: Smo (ice) = 37.99 J K-1 mol-1 Smo (water liquid) = 69.91 J K-1 mol-1