The equilibrium constant for the dissociation of O, into atomic oxygen, 02 = 20 %3D at 3000 K is: Kea = 0.0127 Find the equilibrium mole fraction atomic oxygen in air at 3000 K, 1 atm. Assume no other reactions occur and the gases are ideal. Repeat at 3000 K, 100 atm.
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- Calculating Thermodynamic Values from an Equilibrium ConstantBackgroundAs discussed in lecture, the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion…10. The thermodynamic functions for the generic reaction A+B=>C at 25oC are: ΔH=-35.7 kJ/mole; ΔS=-6.95 J/mole*K Calculate ΔG in kJ/mole Group of answer choices 146 -37.7 -35.5 -33.6 2036Consider a hypothetical gas-phase reaction A + B ⇔ C for which ∆G◦ = −10.00 kJ mol at 298.15 K. Assume that the gases are ideal. a. Find the value of (∂G /∂ξ ) T ,P if PA = 1.00 bar, PB = 0.500 bar, and PC = 0.250 bar. b. Find the value of the equilibrium constant. c. If the initial partial pressures are those in part a, find the equilibrium values of the partial pressures.
- Q1 You wish to design an effusion source for Br atoms from Br2(g). Br2 (g) ⇄ 2Br (g) If the source is to operate at a total pressure of 0.0132 bar at 1000 K, what is the value of the equilibrium constant if the degree of dissociation is 0.35? What pressure is required to increase the degree of dissociation to 0.75 at same temperature? Is this consistent with LeChatelier’s principle? Explain. Plz solve all and Asap...!In the gas-phase reaction A + B ⇋ C + 2 D, it was found that, when 2.00 mol A, 1.00 mol B, and 3.00 mol D were mixed and allowed to come to equilibrium at 25 °C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate (i) the mole fractions of each species at equilibrium, (ii) K, and (iii) ΔrG⦵.The following reaction presents a ΔH0 and ΔG0 of 217.9 kJ/mol and 72.4 kJ/mol respectively, at 600 K. Calculate the temperature necessary for the equilibrium constant being 26. Comment on the approximations you assumed.
- At T = 298.15 K, the equilibrium constant of a reaction is 3.876926675 x 10-6. What is the equilibrium constant at T = 305.15 K if Hrxn at 293.15 K to 323.15 K is equal to -23.40 kJ/mol?The equilibrium constant of a reaction is found to fit the expression lnK = A + B/T + C/T3 between 400 and 500 K with A = -2.04, B = -1176 K, and C = 2.1x107 K3. Calculate the standard reaction enthalpy and standard reaction entropy at 450 K.(a) Under what conditions is a dA < 0 condition thatdefines the spontaneity of a process?(b) A sample containing 2.50 moles of He (1 bar, 350. K) ismixed with 1.75 mol of Ne (1 bar, 350. K) and 1.50 mol ofAr (1 bar, 350. K). Calculate AGmixing and ASmixing.
- at equilibrium, the system CO2 + H2 = CO + H2O has this volume composition 22% CO2, 17% CO, 41% H2 and 20% H2O. Calculate the pressure constant Kp for this reaction at 1900K and 98501Pab) In a company that wants to use this gas equilibrium as a source of hydrogen gas H2, it is desired with a gas pressure of hydrogen equal to 7,850 atm. What equilibrium pressure in atm of ethanol C2H5OH is required to satisfy this requirement? c) What must the initial pressure of ethanol be to meet the requirement for 7,850 atm H2 gas at equilibrium? Supplied: Use an S E L table to organize data and set up the expression for Kc after Guldberg-Waages mass action law for the homogeneous gas equilibrium if possible, I would like handwritten answers with calculations. Thanks :)Using the table showing partial pressures for the formation of ammonia and corresponding equilibrium constants, show that at 101 bar, apparent equilibrium constants equals 0.0072 and the thermodynamic equilibrium constant equals 0.0064. please help me. thank you