Why do people still use the mole (unit) in chemistry?
If you added 1 mL of each, same problem and compounded by differences in density. Since mole is a per molecule measurement, it allows you to make real comparisons between compounds. For example 1 mole of acetic acid will have the same number of molecules as 1 mole of stearic acid even though the weights, volumes, and phases might be different.
Why is the mole a unit of measurement? - Chemistry Stack Exchange
2013年6月16日 · $\begingroup$ @matt_black (ii)My reasoning behind all of this was to try to understand why the amount of substance is usually regarded as a dimensional quantity with the mole being its SI unit – a dimensional unit – unlike the dozen which is regarded as dimensionless. And that was my answer – if mole is dimensional then it cannot be just ...
mole - Why are osmoles not considered SI units? - Chemistry …
2016年6月20日 · Maybe because "osmole" has the same measurement units as "mole" and the latter is the SI unit with that measurement unit. For example, one mole of sodium chloride gives two osmoles in water solution; the conversion between them is . $2$ osmol/mol. showing the two quantities have the same measurement unit. The mole was included into the SI ...
mole - What is the dimension of molar mass? - Chemistry Stack …
2022年1月3日 · $\begingroup$ Using the current official definition, you should not substitute a dimensionless number for the unit mole. A dozen is equal to 12, but a mole is not equal to the Avogadro number in the SI unit system. Thus, g/mol and Da are not equal in the SI system, and the given equation is incorrect.
mole - amu and g/mol relation - Chemistry Stack Exchange
2014年6月20日 · The Avogadro number is the (dimensionless) ratio of one gram to one "atomic mass unit" (now called dalton, Da): g/Da. One mole is an an Avogadro number of entities: mol = (g/Da) ent. Thus we have the important relationship: Da/ent = g/mol = kg/kmol, exactly.
The mole is used extensively in chemistry, why not elsewhere?
2012年6月21日 · The mole is useful in chemistry because it relates two popular but inconsistent units of mass - the atomic mass unit (u) and the gram. One mole of atoms of an element with atomic mass x u, has a mass of x grams. We don't use atomic mass units outside chemistry, so we also have no need for the mole.
What exactly is a mole? - Chemistry Stack Exchange
2016年10月11日 · The first thing to realize is that "mole" is not a mass unit. It is simply a quantity - a number - like dozen or gross or score. Just as a dozen eggs is 12 eggs, a mole of glucose is $6.02 \times 10^{23}$ glucose molecules, and a mole of …
What is the intuition behind 'mol' as a unit 'symbol'
2020年10月12日 · The mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon 12; its symbol is "mol". When the mole is used, the elementary entities must be specified and may be atoms, molecules, ions, electrons, other particles, or specified groups of such particles.
Conversion of a value between g/gmol and lb/lbmol
The mole is a unit of numberical count. Like a dozen is twelve unit entities (eg. twelve eggs in a dozen eggs), 1 mol is shorthand for 6.022x10^23 counted units of the substance as elementary entities (eg. photons, electrons, He atoms, H2O molecules...). A box with one mole of H2O in it has 6.0221x10^23 H2O molecules in it. A mole is just a number.
Is “amount of substance” the same thing as “number of moles”?
2017年5月28日 · A mole is simply defined as "Avogadro number" of something. That is, 1 mole of (say) carbon atoms is about $6.02\times10^{23}$ carbon atoms. Both have a dimension of 1 (the number one); a mole is conveniently represented as a unit of measurement but doesn't actually hold any physical meaning.