A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar and a NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) for mixture 1 at 298 K. please give solution and answer
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A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar and
a NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) for
mixture 1 at 298 K.
please give solution and answer
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- A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar anda NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) formixture 1 at 298 K. A second reaction mixture (mixture 2) is prepared at 298 K with a N2O4(g) partialpressure of 0.05 bar and a NO2(g) partial pressure of 0.10 bar. (i) Calculate the reaction Gibbs energy (∆??) for mixture 2 at 298 K. (ii) Comment on the spontaneity of the forward reaction for mixture 1 and mixture 2.Support your answer with the values of ∆?? calculated for the two mixtures. please give solution and answerThe equilibrium constant of the reaction 2 C3H6 (g) ⇌ C2H4(g) + C4H8(g) is found to fit the expression InK= -1.04-(1088 K)/T +(1.51 x 10-2 K2)/T2between 300 K and 600 K. (a) Calculate the standard reaction Gibbs energy at each temperature at 390 K and 410 K. (b) Use the van 't Hoff equation to determine the standard reaction enthalpy at 400 K. (c) Hence also calculate the standard reaction entropy at 400 K.The standard Gibbs energy of reaction at 721 K for the reaction H2(g) + I2(g) -> 2 HI(g) is ─23.6 kJ. What is the Gibbs energy at 721 K of the following reaction mixtures a) wherein the partial pressure of H2(g), I2(g) and HI(g) are 2.1 bar, 1.7 bar and 1.2- bar, respectively? b) wherein the partial pressure of H2(g), I2(g) and HI(g) are 0.62 bar, 0.23 bar and 3.2 bar, respectively? c) Interpret the results obtained for the two cases. Answer: [─29.0; +2.05]
- For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar anda NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) formixture 1 at 298 K. please give answer and solutionPhysical Chemistry: Show complete solution. a) Find the equilibrium constant at 298.15 K for the reactionN2(g) + H2(g) ⇌ 2NH3(g), ΔG° = -32.734 kJ/mole b) Find the equilibrium composition (in terms of pressure) of a system originally consisting of 0.25 mol N2 and 0.75 mol H2 maintained at 298.15 K and 1 atm.
- For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium? ....... J/mol The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 68 oC is Keq = 401,568. (b) What is the standard reaction Gibbs energy of this reaction?.....J/molCalculate the standard Gibbs energy change for the following reaction at 298 K H2(g) + Cl2(g) ® 2HCl(g) [DfHo = –92.3 kJ mol–1 for HCl; S in J K–1 mol–1 is 131, 223, and 187 for H2, Cl2 and HCl, respectively].[References) At 1100 K, K, = 0.18 for the reaction %3D 2802 (g) + O2 (g) 2S03 (g) What is the value of K at this temperature?
- ST5G.2 - Estimate the solubility of CaF2(aq) [in units of PICOmolar] in the presence of 0.701 molar AIF3(aq). [This is a bit fictitious - I don't think aluminum fluoride is soluble, but I want you to think carefully about the fluoride concentration.] Type your answer..Basing on the standard Gibbs energy of formation, determine if the hydrogenation of benzene to cyclohexane, i.e. C6H6(1) + 3 H2(g) →→ C6H12(1) is feasible. [-97.8] Standard Gibbs energy of formation, in kJ mol-¹, at 25°C Benzene, C6H6(1) + 124.5 Carbon dioxide, CO₂(g) - 394.4 Carbon monoxide, CO(g) - 137.2 Cyclohexane, C6H12(1) + 26.7 Ethanoic acid, CH3COOH (1) - 299.8 Ethanol, C₂H5OH(1) - 174.8 Water, H₂O(1) -237.1For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.