The molecular formula of water is H2O.
The Atomic Mass of H2O is 2(1.0) + 16.0 = 18.0Amount of H2O = mass of pure sample/molar mass = 75/18.0 = 4.17mol
There are 4.17 moles of water in a 75 gram pure sample.
72g/18g=4 moles
0.5002 moles.
36 grams of water have 2 moles
72,08 g of H2O is equal to moles.
5,1 moles
It forms H2O when burned.There are 3.744 moles of H2O after burned.
2.95 mole H2O (2 moles H/1 mole H2O) = 5.90 moles hydrogen ------------------------------
There is no nitrogen in water.
Two moles of water are produced.
6,49 moles of water are obtained.
6.49 moles of water
H2O or water doesn't have any helium in it.
It forms H2O when burned.There are 3.744 moles of H2O after burned.
3.2 moles of water (H2O)
2.95 mole H2O (2 moles H/1 mole H2O) = 5.90 moles hydrogen ------------------------------
According to this balanced equation:Na2O + H2O --> 2NaOH42 moles Na2O react with 42 moles H2O
0.943 moles H2O (6.022 X 1023/1 mole H2O) = 5.68 X 1023 molecules of water ========================
There is no nitrogen in water.
Two moles of water are produced.
Sulfuric acid is not obtained from water.
6,49 moles of water are obtained.
6.00 g H2O x 1 mol H2O/18 g H2O = 0.333 moles of water present in 6.00 g of water. How anyone came up with 3.00 moles is a mystery.