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# Does this give molar mass?

https://fbcdn-sphotos-h-a.akamaihd.net/hphotos-ak-...

Or is the 1 mol/1 mol redundant?

If it's wrong can you show me how to do the correct units

Thanks! ☺

When I do this: https://fbcdn-sphotos-h-a.akamaihd.net/hphotos-ak-...

I think I get mole/L and if I multiply that whole equation by mol/mol i get the moles.

Can the mol/l be the same as mol?

Thanks

When I do this: https://fbcdn-sphotos-h-a.akamaihd.net/hphotos-ak-...

I think I get mole/L and if I multiply that whole equation by mol/mol i get the moles.

Can the mol/l be the same as mol?

Thanks

### 1 Answer

- pisgahchemistLv 77 years agoFavorite Answer
It would appear that this is supposed to compute a molar mass when 0.607g of solute is dissolved in 0.0276 L of a solution with a concentration of 0.3922 mol / L.

Here is the proper way to set it up.

(0.607g / 0.0276 L) x (1 L / 0.3922 mol) = 56.1 g / mol

Use the reciprocal of the concentration as a conversion factor which cancels out "liters" and places "mol" in the denominator. The (1 mol / 1 mol) would be superfluous. The real problem is that there is one too many "L". The ratio "1L / 0.0276 mol/L" is the same as saying "L² / 0.0276 mol".