Answer:
The molar mass of lysine using the ideal gas equation for this problem is 146.25 g/mole.
Explanation:
The ideal gas equation PV = nRT, was derived from the ABC laws (Avogadros, Boyles and Charles laws). We need to obtain the value for the number of moles n.
The parameters of this equation are:
P = 1.918 atm
V = 750.0mL = 0.75L
n = ?
R = 0.0821
T = 25 degree celcius = 25 + 273 = 298 degree kelvin.
From this formular, n = (PV)/(RT)
n = (1.918 X 0.75)/(0.0821 X 298 )
n = 0.0588
n, no of mole = mass/molar mass
0.0588 = 8.6/MM
MM = 8.6/0.0588
MM = 146.25g/mole.
Answer:
Molar mass of lysine is 146.267 grams per mole.
Explanation:
Osmotic pressure(π) is given by the formula
π = cRT
where c is concentration in [tex]\frac{moles}{L}[/tex] (Molarity).
c = no of moles per volume in litres.
R is universal gas constant = 0.0821 [tex]\frac{L-atm}{mole-K}[/tex]
T is temperature in K.
Substituting values in the above equation gives
1.918 = [tex]\frac{8.6\times1000}{M\times750}\times0.0821\times298[/tex]
M = 146.267 grams per mole.
