In chemistry, a mole is actually a unit of measurement, like an inch, meter, or gram. It is 6.02 x 10^23 of something, usually atoms or molecules. For example, one mole of Hydrogen would contain 6.02 x 10^23 atoms of Hydrogen.
For example:
Mix a kilogram of tablesalt with a kilogram of glucose.
What is the mole percentage of glucose in this mixture?
MM NaCL = 58.443 g/mol
MM C6H12O6 = 180.1566 g/mol
1000 g / 58.44 g/mol = 17.11 mole
1000 g / 180.16 g/mol = 5.55 mole
Total is 17.11 + 5.55 = 22.66 mole
The mole percentage of glucose is 5.55 / 22.66 * 100 = 24.49%
So eventhough the mass percentage is 50%, the mole percentage is not.
This is important in determening the right amount of chemicals to add together in experiments. if a reaction says: 1x + 1y --> 1xy
and you add 1 kg x to 1 kg y, you will have 1 of these reactants in excess and you wont have as much of the product as you wanted to have.
One mole (6.023× 1023) is the amount of a pure substance
containing the same number of chemical units, as there are atoms in exactly 12 grams of carbon-12 (i.e. 6.023
×
1023).
One mole of water is equal to 18 grams of water, which is equal to 18 ml of water. (1gram=1ml of water)
6.02*10^23
We assume 100 grams of compound and change % to grams. Get moles. 40 grams S (1 mole S/32.07 grams) = 1.247 60 grams O (1 mole O/16.0 grams) = 3.75 Now, the smallest mole value, sulfur, is 1. Divide the oxygen mole value by the sulfur mole value. 3.75 mole O/1.247 mole S = 3.00 SO3 ------- is the empirical formula
50% of 64 g compound XX = 32, so 32 g S = 1.0 mole S 50% of 64 g compound XX = 32, so 32 g O2 = 1.0 mole O2 or =2.0 mole O atoms Thus it is SO2
We assume 100 grams total and turn those percentages into grams. Get moles elements. 29.6 grams O (1 mole O/16.0 grams) = 1.85 mole O 70.4 grams F (1 mole F/19.0 grams) = 3.71 mole F now divide both moles by smallest number to get mole ratio for empirical formula 1.85/1.85 = 1 for O 3.71/1.85 = 2 for F so the empirical formula for this compound is........ OF2
mole mole mole mole mole
1 mole of oxygen contains 6.022 x 1023 atoms. A mole of atoms of any element is 6.022 x 1023 atoms. A mole of anything is 6.022 x 1023 of that thing. For example, a mole of cars is 6.022 x1023 cars.
No.
1 mole =how much ppm
.005078 g is the weight of 2 mole percent molecular iodine.
The mole fraction of HCl in 20 percent aqueous solution is 0.21.
No, the two concepts are quite unrelated.
Mole percent, or molar percent of a substance is the ratio of the moles of a substance in a mixture to the moles of the mixture. It represents the number of moles of a substance in a mixture as a percentage of the the total number of moles in the mixture. Mole % = (mol substance in a mixture) / (mol mixture) * 100
the mole fraction of oxygen= 37/100 0.37 the mole fraction of Nitrogen= .63 that equals to give 1
You need the balanced symbol equation for the reaction. The numbers in front of the formulae show the mole ratios. For example, in the thermal decomposition of calcium carbonate: CaCO3 --> CaO + CO2 The equation is balanced. The mole ratio between CaCO3 and CO2 is 1:1 because there is 1 mole of CaCO3 for every mole of CO2
The mole fraction of HCl is 0.34.
Yes - as long as the pressure and temperature are constant.
We assume 100 grams of compound and change % to grams. Get moles. 40 grams S (1 mole S/32.07 grams) = 1.247 60 grams O (1 mole O/16.0 grams) = 3.75 Now, the smallest mole value, sulfur, is 1. Divide the oxygen mole value by the sulfur mole value. 3.75 mole O/1.247 mole S = 3.00 SO3 ------- is the empirical formula
multiply the esoteric value by the mole fraction of the color of the moon