First you find the Molar Mass of water using the values on the Periodic Table.
2 Hydrogen + 1 Oxygen
2*1.01 + 16.00 = 18.02 g/mol
Then using factor-label to cancel out units
(100g H2O)*(1 mol H2O / 18.02 g H2O) = 5.54938957 mol
So the number of moles in 100g of H2O is about 5.55 moles.
Hope that helps.
1 molecule of water is composed of:
H2, with a molar mass of 2.02g, assuming 3 significant digits.
O, with a molar mass of 16.0g, assuming 3 significant digits.
Therefore, 1 mole of water (H2O) molecules has a mass of 18.0g, keeping 3 significant digits.
Then you just divide 100g by 18g, getting 5.555555...
You must keep the 3 significant digits from before, though, so you round to 5.56.
Your answer is 5.56 moles of water (H2O) in 100 grams of water (H2O).
For this you need the atomic (molecular) mass of H2O. Take the number of grams and divide it by the Atomic Mass. Multiply by one mole for units to cancel. H2O=18.0 grams
100.0 grams H2O / (18.0 grams) =5.56 moles H2O
Formula of water = H2O Relative atomic mass of hydrogen = 1
Relative atomic mass of oxygen = 16
Relative molecular mass of H2O = 1 + 1 + 16 = 18
Moles = mass of substance/relative molecular mass
Moles = 100/18
Moles of water in 100g = 5 and 4/9 moles or approximately 5.56 moles
100 grams water (1 mole H2O/18.016 grams)
= 5.55 moles of water
================
100 grams water (1 mole H2O/18.016 grams)(2 moles H/1 mole H2O)
= 11.1 moles of hydrogen
==================
100 grams of H2O is equal to 5,555 moles.
95,474 moles
== == Nickel (II) and Nickel (III) have the same behaviors.I couldn't find any information at all on Ni(III) chlorate, but I did find this on Ni(II)ClO3. The +2 oxidation state of Ni is much more common. Molar percent concentration: At 0 °C, solubility is 8.88 moles per 100 moles water, and at 25 °C, 12.02 moles per 100 moles water. Mass percent concentration: At 0 °C: 111 grams per 100 grams water At 20 °C: 133 grams per 100 grams water At 80 °C: 308 grams per 100 grams water See the related links for the source (Google Books).
No. of moles=wt. of substance/molecular wt. hence, wt. of substance= 2.38*100=238
C2H4O2 + NaOH = H2O + C2H3O2Na Acetic acid (60 gm) + sodium hydroxide ( 40 gm) = 100 gm water (18 gm) + sodium acetate (82 gm) = 100 gm Ratio reactants to products = 1:1 Molarity = moles / L, 3M = 3 moles / 1 L Acetic acid = 60 gm / total reactant 100gm = 1.8 moles Multiply by 3 = 1.8 moles or 180 grams Sodium Hydroxide = 40 gm / total reactant 100 mg = 1.2 moles or 120 grams. 180 grams acetic acid + 120 grams sodium hydroxide = 300 grams. 300 grams divided by 1 liter = 3M So in order to make 3 M sodium acetate combine solution, add 180 grams acetic acid and 120 grams sodium hydroxide with 1 liter of water.
20
if you have 100 liters how many moles does that equal?
95,474 moles
4.00
== == Nickel (II) and Nickel (III) have the same behaviors.I couldn't find any information at all on Ni(III) chlorate, but I did find this on Ni(II)ClO3. The +2 oxidation state of Ni is much more common. Molar percent concentration: At 0 °C, solubility is 8.88 moles per 100 moles water, and at 25 °C, 12.02 moles per 100 moles water. Mass percent concentration: At 0 °C: 111 grams per 100 grams water At 20 °C: 133 grams per 100 grams water At 80 °C: 308 grams per 100 grams water See the related links for the source (Google Books).
100 grams MgCO3 (1mol MgCO3/84.32g) = 1.19 moles of MgCO3
100 grams
100 grams of water is approximately 20 teaspoons
For this you need the atomic (molecular) mass of NH3. Take the number of moles and multiply it by the atomic mass. Divide by one mole for units to cancel. NH3=16.0 grams100 grams NH3 / (16.0 grams) = 6.25 moles NH3
The answer depends on the temperature, but at room temperature (20 deg C), 100 ml of water would have a mass of 99.82 grams.
No. of moles=wt. of substance/molecular wt. hence, wt. of substance= 2.38*100=238
K2CrO4 Molarity (concentration) = moles of solute/Liters of solution (100 ml = 0.100 Liters ) Find moles K2CrO4 first. 3.50 grams = (1 mole K2CrO4/194.2 grams) = 0.01802 moles K2CrO4 ----------------------------------------------next Molarity = 0.01802 moles K2CrO4/0.100 Liters = 0.180 M K2CrO4 -------------------------
100 grams oxygen (1 mole O/16 grams)(2 mole Fe/3 mole O) = 4.17 moles iron --------------------------