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# Commercial sample of ammonia has density of 0.91g/cm3  and has 25 % Ammonia on  weight by weight basis.  Calculate a) Molarity and mole fraction of ammonia  b) Volume of this NH3 required to prepare 3000 cm3  of 1M NH3.  (5) Q.2) How did van der Waals’ make amendments in the Ideal Gas Equation in order to  make it valid for real gases? (5) Q.3) Draw the crystal structure of NaCl

Asked by tanvitakle22 24th October 2018, 8:49 PM
Molarity = 10 × %c × d /Molar mass = 10 × 25 × 0.91 /17 = 13.38M

Mole fraction ; Weight of solute = 25 × 100 = 2500g so number of moles = 2500/17 = 147moles

mole fraction = {147/147 + 1.47) = 147/148.47 = 0.99

b) use M1V1 = M2V2 = 13.38 × V = 1 × 3 or V = 3/13.38 = 0.22L (since 3000cc = 3L)

2  Vanderwaal added pressure correction and reduced volume correction from the ideal pressure and volume of ideal gas equation

3)
Answered by Expert 31st October 2018, 1:56 AM
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