A2.550 x 10^−2 m solution of glycerol (c3h8o3) in water is at 20.0°c. the sample was created by dissolving a sample of c3h8o3 in water and then bringing the volume up to 1.000 l. it was determined that the volume of water needed to do this was 998.9 ml . the density of water at 20.0°c is 0.9982 g/ml.
a. calculate the molality of the glycerol solution.

Explanation:

Given , molarity of glycerol=

Volume= 1 L.

Therefore, No of moles of glycerol=

Now, volume of water needed, V=998.8 mL.

Density is given as= 0.9982 g/mL.

Therefore, mass of water =

Now, molality=

Hence, this is the required solution.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.