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An oblong number is a composite (non-prime) number. If p and q are a factor-pair for an oblong number n, then the number n can be represented by a rectangle or oblong that is p units x q units.
It depends on the substance and its molar mass.In order to convert from grams to formula units, you must first convert grams to moles, then moles to formula units (grams --> moles --> formula units).1. Divide the mass (g) of the given substance by the substance's molar mass.2. Multiply the number of moles found in Step 1 (above) by Avogadro's number (6.022 x 1023).---- Mass substance ----- X 6.022 x 1023 formula unitsMolar mass substanceCONVERSION FACTOR47.63g substance x 1 mol substance ---- x ----- Avogadro's number///////////////////// molar mass (g) substance ////// 1 mol substance
Any metric or non-metric units can be represented by points on the plotted line.
If your bank account is overdrawn by 5 units then your statement will show the balance as -5. So the negative number, -5, is represented as a debt of 5 units of currency (an absolute number).
You need to know that one mole is 6.022 x 1023 particles (atoms, molecules, ions, formula units, etc...).
It represents the amount of the substance. It can mean the number of atoms, molecules, formula units, or moles.
A coefficient is a number written in front of a chemical formula when balancing a chemical equation. The coefficient can represent the number of atoms, molecules, formula units, or moles of the substance.
0.688 moles*6.02x1023=4.14x1023 Formula units
The volume occupied by 2.12 moles of nitrous oxide is 9.35. A mole is described in chemistry as an amount of pure substance containing the same number of chemical units as there are atoms.
The number of moles is 1,8.
The number of units indicated by each description of moles of atoms and moles of molecules is the same and is specifically Avogadro's Number, about 6.022 X 10^23
You don't need to use Avogadro's number, you need the mass of the molecule in atomic units. Mass / molecular mass = moles eg for water, 36 grams / 18 atomic units = 2 moles
FORMULA UNITS TO MOLES (formula units --> moles)Divide the number of formula units by Avogadro's number.----------- Formula UnitsAvogadro's number (formula units)Conversion FactorFormula Units x 1 mol-------- Avogadro's number (formula units)MOLES TO FORMULA UNITS (moles --> formula units)Multiply the number of moles by Avogadro's number.Moles Substance x Avogadro's numberConversion FactorMol substance x Avogadro's number---------------------- 1 mol substanceMOLES TO GRAMS (moles --> grams)*Multiply the number of moles by the substance's molar mass.Moles Substance x Molar Mass SubstanceConversion FactorMol Substance x Molar Mass Substance------------------------- 1 mol SubstanceGRAMS TO MOLES (grams --> moles)*Divide the number of grams by the substance's molar mass.---- Mass (g) SubstanceMolar Mass (g) SubstanceConversion FactorMass (g) Substance x 1 mol substance----------------------- Molar Mass Substance (g)FORMULA UNITS TO GRAMS (formula units --> moles --> grams)*Divide formula units by Avogadro's number (6.022 x 1023 formula units); multiply by molar mass.--- Formula Units --- x --- Molar MassAvogadro's numberConversion FactorFormula Units x 1 mol ----------------- x -------------- Molar mass (g)---------- Avogadro's number (formula units) ----------- 1 molGRAMS TO FORMULA UNITS (grams --> moles --> formula units)*Divide mass of substance by the molar mass of substance; multiply by Avogadro's number.---- Mass (g) substance -- x -- 6.022 x 1023 moleculesMolar mass (g) substanceConversion Factor--- Mass substance (g) x 1 mol substance ------ x ----- Avogadro's number------------------------ Molar Mass (g) substance ----------- 1 mol substanceTip: On test day, anytime you see the words ions, formula units, molecules, or atoms on a question, that problem will involve the usage of Avogadro's number.*Finding Molar Mass# Atoms Element A x Atomic Mass Element A (Periodic Table) = mass (g) El. A# Atoms Element B x Atomic Mass Element B (Periodic Table) = mass (g) El. B... etc.Add up all the mass values found above and you have molar mass.
We convert units to moles because in reactions atoms of different elements combine in simple whole-number ratios. The whole numbers are related to the number of atoms, not their weights.
5.68 mol MgO x 6.02E23 formula units / 1 mol = 3.42E24 Formula Units
moles
One mole of formula units = 6.022 x 1023 formula units.