A gaseous compound has a density of 1.87 g/L at 26.8 °C and 1.83 atm. What is the molar mass of the compound? molar mass:

25.15g/mol

Explanation:

To solve this question, we say

PV = nRTformula 1

Where P= pressure = 1.83atm

V = volume

n= number of moles

R = General gas constant = 0.0821 Latm/Kmol

T = Temperature = 26.8 + 273 = 299.8K

However, Density (D) = number of moles (n) / volume (V) formula 2

Also, number of moles (n) = mass (m) / molar mass (MM)formula 3

- Rearranging the formula 2, we have:

mole (m) = density × volume

- Rearranging formula 3, we have:

mass (m) = molar mass × moles

This means that;

Density = mole × molar mass/volume

Volume = number of moles (n) × molar mass(MM) / density(d)

Inserting into PV=nRT

PnMM/d = nRT

Divide both sides by n

PMM/d = RT

Molar mass (MM) = D.R.T / P

Molar mass = 1.87 × 0.0821 × 299.8 / 1.83

Molar mass = 46.0273946/1.83

Molar mass = 25.15g/mol

to make a supersaturated solution, make a saturated solution of sugar by adding 360 grams of sugar to 100 ml of water at 80 degrees celsius. when the water cools back down to 25 degrees, that 360 grams of sugar will still be dissolved even though the water should only dissolve 210 grams of sugar.