1 liter of (liquid) water contains 55.5 moles.
1 litre of water contain 55,55 moles.
6.
7 if it is saltwater.
22.4 liters at STP
1 L water contain 55,55 moles.
Well the definition of molarity is how many moles in every litre. You already have your answer expressed as moles in a litre, approximately. Density is approximately 1000g per litre, therefore it will be approximately 2 molar. (You haven't expressed temperature, but density should remain close to 1).
The number of moles is 0,527.
The moles number of water 12; the chemical formula is KAl(SO4)2.12H2O.
2,000,000,000,000,000 moles
54,0 grams of water is equivalent to 3 moles.
2.3M means 2.3 moles per litre. Number of moles = 2.3mol/litre x 0.630litre = 1.449mols
Roughly zero. One litre is more water than I can drink in one go, and 0.82 moles of water is too small to see.
Assume purity unless otherwise stated. Find out the density and apply it to 1 litre to find out how many grams a litre will weigh. divide this answer by the molecular weight to get the number of moles in a litre
Well the definition of molarity is how many moles in every litre. You already have your answer expressed as moles in a litre, approximately. Density is approximately 1000g per litre, therefore it will be approximately 2 molar. (You haven't expressed temperature, but density should remain close to 1).
The number of moles is 0,527.
The answer is 6 moles.
6.49 moles of water
9.991 Moles (water) 8.982 Moles (heavy water)
The moles number of water 12; the chemical formula is KAl(SO4)2.12H2O.
2,000,000,000,000,000 moles
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.
A number of atoms/molecules in a given number of moles is regardless of the substance unless it deals with stoicheometry. One mole represents a number of Avogadro's constant, approximately 6.022 x 10^23. Therefore there are 1.91 x 10^25 molecules of water in 31.8 moles.