At RT i.e. 25 C, the density of water is 1 g/L.
Mass of water = Density x volume = 1 g/L x 0.0018 x 10-3 L = 1.8 x 10-3 g
18 g water = 1 mole
1mole water contains 6.023 x 1023 molecules of water
So, 18 g water cotains 6.023 x 1023 molecules of water
Then, 1.8 x 10-3 g water contains 1.8 x 10-3 x 6.023 x 1023 / 18 g = 6.023 x 1019 molecules of water
===>> 6.023 x 1019
At RT i.e. 25 C, the density of water is 1 g/L.
Mass of water = Density x volume = 1 g/L x 0.0018 x 10^-3 L = 1.8 x 10^-3 g
18 g water = 1 mole
1mole water contains 6.023 x 1023 molecules of water
So, 18 g water cotains 6.023 x 1023 molecules of water
Then, 1.8 x 10^-3 g water contains 1.8 x 10^-3 x 6.023 x 1023 / 18 g = 6.023 x 10^19 molecules of water
===>> 6.023 x 10^19
can someone explain?
At RT i.e. 25 C, the density of water is 1 g/L.
Mass of water = Density x volume = 1 g/L x 0.0018 x 10^-3 L = 1.8 x 10^-3 g
18 g water = 1 mole
1mole water contains 6.023 x 1023 molecules of water
So, 18 g water cotains 6.023 x 1023 molecules of water
Then, 1.8 x 10^-3 g water contains 1.8 x 10^-3 x 6.023 x 1023 / 18 g = 6.023 x 10^19 molecules of water
===>> 6.023 x 10^19