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step 1; find # of moles
1.00*10^24 molecules x 1 mole of 6.02*10^23 molecules = 8.52*10^17 mole of H2O
( 1.0010*10^24 x 6.02*10^23 )
= 8.52*10^17
step 2 ; mass of H2O
8.52*10^17 mole x 18.02 grams per mole = 1.18*10^17 g H2O
( 8.52*10^17 x 18.02 )
= 1.18*10^17
Wiki User
∙ 13y ago
Wiki User
∙ 12y agoOne and a partial molecule? You asked for it.
1.001024 molecules of water (1 mole H2O/6.022 X 10^23)(18.016 grams/1 mole H2O)
= 2.994761 X 10^-23 grams
-----------------------------------------( a negligible mass!! )
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What would be the Mass of 3 moles of ammonia and calculate the number of ammonia molecules?
The mass of 3 mol of ammonia is 51,093 g; the number of ammonia molecules in 3 moles is18,066422571.10e23.
Why does the volume of the water vapor increase and the mass remain constant When 1 gram of water is evaporated?
Mass is mass. It is constant. Changing water from liquid to gas does not change the mass, it only changes the density, which is mass per volume. Look at it another way - in gaseous form, the same mass of water has the same number of molecules of water - but those molecules are simply further apart.
How many molecules are in 12.5g of water?
The molar mass of water (H2O) is approximately 18 g/mol. To calculate the number of molecules in 12.5 g of water, we need to convert grams to moles by dividing by the molar mass. 12.5 g / 18 g/mol = 0.694 moles. Since 1 mole of any substance contains 6.022 x 10^23 molecules (Avogadro's number), multiplying 0.694 moles by Avogadro's number gives us approximately 4.18 x 10^23 molecules of water in 12.5 g.
Is it always true that the molecules of dense liquid are heavier than the molecules of lighter molecules?
NO. Water has a density greater than gasoline, but gasoline, octane anyway, has a greater molecular mass than water molecules.
How do water molecules in the solid phase compare with water molecules in the gaseous phase?
if you are awesome like casy connor anthony
How can you demonstrate ther is space between molecules of water?
Calculate volume of molecule, calculate mass of molecule, compare to bulk density. Lower bulk density indicates empty space.
Does ice molecules has less mass than water molecules?
no it has more
What would be the Mass of 3 moles of ammonia and calculate the number of ammonia molecules?
The mass of 3 mol of ammonia is 51,093 g; the number of ammonia molecules in 3 moles is18,066422571.10e23.
Does changing the mass of water change the mass of one cubic centimeter of water?
You can change the mass of water in two ways: increase or decrease the amount of water or change the isotopic composition of the molecules of water. The first will have no effect on the mass of 1 cc of water. The second will. If you replace the hydrogen atoms in the "normal" water molecules with deuterium atoms you will increase the density (mass/cc) of the water.
How do you calculate specific heat?
Change in mass -------------------- Change of water That is change in mass divided by change of water
Why does the volume of the water vapor increase and the mass remain constant When 1 gram of water is evaporated?
Mass is mass. It is constant. Changing water from liquid to gas does not change the mass, it only changes the density, which is mass per volume. Look at it another way - in gaseous form, the same mass of water has the same number of molecules of water - but those molecules are simply further apart.
Which one has more molecules 9 g of water or 9 g of suger (C12 H22 O11)?
Since the molecular mass of water is about 18 and the molecular mass of C12H22O11 is about 342, it takes considerably more molecules of water to make up 9 g than molecules of C12H22O11 to get the same mass.
What is the theoretical percentage of water of hydration in cacl2-2h20?
1. Find the molar mass of the hydrate (Calcium Chloride Dihydrate).Find the molar mass of water and the anhydrate (anhydrate + water = hydrate); add the molar mass values of each to find the molar mass of the hydrate.Molar Mass CaCl2: 110.98g+ Molar Mass H2O: 36.04g*Molar Mass CaCl2 * 2H2O: 147.01gFinding Molar Mass# atoms element A * atomic mass element A = Mass A# atoms element B * atomic mass element B = Mass B... etc.Add up all the mass values and you have the value for molar mass. Do this for both the anhydrate and the water molecules. Add these values together to find the molar mass of the hydrate.Molar Mass Anhydrate + Molar Mass Water Molecules* = Molar Mass Hydrate* Tip: the molar mass of water for all hydrate calculations is 18.02g x number of water molecules. This number may be useful to remember on the day of the test or while doing practice problems.*2. Calculate the percentage of water in hydrate.Divide the molar mass of water by the molar mass of the hydrate, and multiply result by 100%.36.04g147.01g x 100%Percent water in hydrate is 24.52%.
When boiling water turns to steam what stays the same?
The mass of the water The number of molecules
How many molecules are in 12.5g of water?
The molar mass of water (H2O) is approximately 18 g/mol. To calculate the number of molecules in 12.5 g of water, we need to convert grams to moles by dividing by the molar mass. 12.5 g / 18 g/mol = 0.694 moles. Since 1 mole of any substance contains 6.022 x 10^23 molecules (Avogadro's number), multiplying 0.694 moles by Avogadro's number gives us approximately 4.18 x 10^23 molecules of water in 12.5 g.
When 1 gram of water is evaporated the volume of the water vapor increases but the mass remains constant Why does the mass of the water remain constant?
There is no way that mass can be created or destroyed. Here is an informal way to consider the situation. When you evaporate the water, the distance between the molecules increases. But no new molecules are created (or destroyed). Well, the mass is not simply the total number of molecules - but this gives you an idea how this situation works.
What is the mass of a single molecule of water?
- calculate the molecular mass of the substance from the atomic weights of the contained elements - 1 molecule gram of any substance contain 6,023 141 79.1023 molecules (Avogadro number) - mass of a single molecule is: Molecular mass in grams/Avogadro number
