O He was always very gauche and urbane in polite society
At STP (standard temperature and pressure) 1 mole of a gas takes up 22.4L
so 2.33/22.4=0.104 mol H2S
Answer: The name of this Hydrate is magnesium sulphate monohydrate.
Explanation:
Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.
a) If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of
= 87.0 g
Mass of
= 13.0 g
Step 1 : convert given masses into moles
Moles of
=![\frac{\text{ given mass }}{\text{ molar mass }}= \frac{67.0g}{120g/mole}=0.56moles](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%7B%20given%20mass%20%7D%7D%7B%5Ctext%7B%20molar%20mass%20%7D%7D%3D%20%5Cfrac%7B67.0g%7D%7B120g%2Fmole%7D%3D0.56moles)
Moles of
=![\frac{\text{ given mass}}{\text{ molar mass}}= \frac{13.0g}{18g/mole}=0.72moles](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%7B%20given%20mass%7D%7D%7B%5Ctext%7B%20molar%20mass%7D%7D%3D%20%5Cfrac%7B13.0g%7D%7B18g%2Fmole%7D%3D0.72moles)
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For
= ![\frac{0.56}{0.56}=1](https://tex.z-dn.net/?f=%5Cfrac%7B0.56%7D%7B0.56%7D%3D1)
For
=![\frac{0.72}{0.56}=1](https://tex.z-dn.net/?f=%5Cfrac%7B0.72%7D%7B0.56%7D%3D1)
Hence the empirical formula is ![MgSO_4.H_2O](https://tex.z-dn.net/?f=MgSO_4.H_2O)
Thus the name is magnesium sulphate monohydrate.