00:01
Knowing the osmotic pressure, we can calculate the molarity.
00:04
This is fairly straightforward using the osmotic pressure equation.
00:09
Rearranging it, the molarity is osmotic pressure divided by r and t.
00:14
The pressure is 10 atmospheres.
00:17
Our r value is 0 .0826 liter atmospheres per kelvin mole.
00:24
And the temperature is 298 kelvin.
00:28
All the units cancel except for liter.
00:30
Per mole in the denominator which become moles per liter in the numerator and we get 0 .42 .994 moles per liter.
00:39
So if we have a liter of this solution, we will have 0 .42 .994 moles of glucose.
00:50
And then if we have this many moles, we'll have a liter and we need to convert the liters into kilograms of just the solvent, assuming the solvent is water, i don't think they tell us it's water, but we're going to have to make that assumption.
01:10
Our liters, we can convert into milliliters.
01:12
We can then use the density of the solution to get the grams of the solution.
01:16
We'll then divide that by 1 ,000 to get kilograms of the solution, but still we are just in units of solution...