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4) A 1.000 L flask is charged with 0.375 moles of gaseous N2O4 which is in...

4) A 1.000 L flask is charged with 0.375 moles of gaseous N2O4 which is in equilibrium with gaseous NO2 with ΔH = 58.02 kJ/mol and ΔS = 176.6 J/(mol*K). What is the pressure in the flask at 300. K? (15 pts) (Hint – Solve for G, solve for K, solve equil. concentrations, and then how many moles of gas are there?)

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☆ solution メーカドー * criven: ③ initiul mole of Ma04 = 0.375 moles volume og flask= 1.000 liter ven thalloy of Reaction - AH = 5Key= equilibrium > Aur = 58.02 X 1095 300 KX 176.6, I moe ~ mol.lt дал - 50405 mol case- Sot Kez and Related ces =) AGE RT Inf cage - 3 ソー given: Rece ction- Ng Oq ef) grlogey fro 0.375 wherer t=toy 0.375.0.3750 9.20.375o a = degree of diego ciation-> ( ng Oq] = 0.395x(1-0) mol liter (11) equilibrium moles of mon e 2 x039564 equilibrium concentration cedeulented are { neosince - given Key = 0.13256 =) 0.13256 1.5.22 (1-0) =) 0.13256 x il-2) = 1-5x22 0.13256- 0,132562 -1.5882 >> 1.529 +0.132562Case - (4 مطر ط & total moles N0.375 x (H) but the value of (&J- ME 0.375*(1+0.95635 =) N = 0.47113 mole from ideal -yas Lane

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