There are 1.5 moles water in 27 grams
Divide mass of 27 g H2O by its molar mass of 18.0 g.mol−1 H2O and you get the number of moles: 1.5 mole H2O
4 moles of oxygen atoms are present in 4 moles of H2O
A mole of water contains avagadro's number of molecules of water. Therefore 5.65 moles contains 5.65 * 6.022x1023 molecules of water which equals 3.40243x1024 molecules of water.
for each mole of anything there is 6.022x10^23 molecules. Therefore for 5 moles of water there is 5 x 6.022x10^23 = 3.011x10^24 molecules of water
Once you have measured out your sample and transferred it to your flask, the absolute amount (moles) of sample is fixed. Adding water to the flask will change the concentration in the flask, titrating also adds volume to the flask as well as reacting with the sample. However, the number of molecules of sample you put into the flask will not change by simply diluting it with water.
3.6 moles hydrogen atoms (1 mole water/2 mole H)(6.022 X 1023/1 mole water molecules) = 1.1 X 1024 molecules of water =======================
Divide mass of 27 g H2O by its molar mass of 18.0 g.mol−1 H2O and you get the number of moles: 1.5 mole H2O
4 moles of oxygen atoms are present in 4 moles of H2O
A mole of water contains avagadro's number of molecules of water. Therefore 5.65 moles contains 5.65 * 6.022x1023 molecules of water which equals 3.40243x1024 molecules of water.
6,022140857.1023 molecules---------------------------------------------1 mole2.1022 molecules--------------------------------------------------------------x molex = 0,033 moles
Your question is irrelevant. I think that you were trying to find the number of molecules present in half a mole of water. 1 mole of water contains 6.023 * 1023 number of molecules. Hence half mole contains half of that number of molecules which is 3.0115*1023.
for each mole of anything there is 6.022x10^23 molecules. Therefore for 5 moles of water there is 5 x 6.022x10^23 = 3.011x10^24 molecules of water
9.991 Moles (water) 8.982 Moles (heavy water)
Assuming a density of 1.0 g/ml for water, then 10 ml H2O = 10 g10 g H2O x 1 mol/18 g = 0.5555 moles H2O0.5555 moles x 6.02x10^23 molecules/mole = 3.34x10^23 molecules of H2O in 10 ml
Once you have measured out your sample and transferred it to your flask, the absolute amount (moles) of sample is fixed. Adding water to the flask will change the concentration in the flask, titrating also adds volume to the flask as well as reacting with the sample. However, the number of molecules of sample you put into the flask will not change by simply diluting it with water.
I am 10
The number of water molecules is 16,728.10e23.