Question

Problem 11.16 5 of 10 > Constants Periodic Table Part A From the corresponding Henry's law coefficient Rx-8.64.10 bar, estimate the molarity of N, (gas) in water at 298 K when the water is in equilibrium with air ata total pressure of 1.14 bar Assume that the air is 78% Ny by volume (Le., by mole number), and that the dissolved Ny does not affect the volume of solution. There are 55.3 moles of water in Lat 298 K Express your answer using two significant figures IVO ANDO ? Submit Request Answ

Answer 1

Henry's Low Igas = kn • xgay Pgay partial pressure above ligued (folution) KH- Henry's constant KH = 8.64 x 10 4 bar Xgay - mole fraction of gay in solution so, Xgas luton h-moly

- An at 1.14bar and it contain __78% by volume (lie. by mole) N2 Soportial pressure of Ng in Air = mole fractionx Protat ingir = 78 x 1.14 * bar lt 100 * [ Png - 0.8892 box - Given that 1L solution contain ss.3 mous of water (solvent) So, het we have 1L folw then moles of H, 0 (tolvent) = 55- 3 mol and moles of N₂ (solute) = ze mol then . mole fraction of N₂ = 2e in solution 55:3+2

Since amount of N, less because it is less soluble to gay in water relatively 55.3 +21 755.3 from Ру = ku• Хя Pre = kn ze 55.3 0.8892 = 8.64 X10 4 x 2 55:3 | 2 = 5:69 x 10-4 moll s.69x 10-4 so, ' IL folution contains moly of N₂ so, * Melanity (M) = 5.69x10-4 M