Respuesta :
The deuteriuoted water that is [tex]D_{2}O[/tex] consists of an isotope of hydrogen in place of hydrogen from the normal water. The approximate mass of deuteriuoted water and normal water can be calculated as {(2×2)+16} = 20. However the exact mass of [tex]D_{2}O[/tex] is 20.027 g/mole, whereas the mass of water can also be calculated as- {(1×2)+16}=18, however the exact mass of ([tex]H_{2}O[/tex]) molecule is 18.015 g/mole. Thus the difference between the mass of the molecules are (20.027 - 18.015) = 2.01 2g/mole.
Answer:
[tex]D_2O[/tex] molecule is greater than [tex]H_2O[/tex] molecule by 2 amu.
Explanation:
Mass of [tex]H_2O[/tex] molecule:
[tex]M_{H_2O} [/tex]= 2 × 1 amu + 1 × 16 amu = 18 amu
Mass of [tex]D_2O[/tex] molecule:
[tex]M_{D_2O} [/tex]= 2 × 2 amu + 1 × 16 amu = 20 amu
Difference between mass of [tex]D_2O \& H_2O[/tex]
[tex]M_{D_2O}-M_{H_2O} =20 amu - 18 amu = 2 amu[/tex]
[tex]M_{D_2O} =2+M_{H_2O} [/tex]
[tex]D_2O[/tex] molecule is greater than [tex]H_2O[/tex] molecule by 2 amu.
