4.3: MoleMass Conversions
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 79551
As described in the previous section, molar mass is expressed as “grams per mole”. The word per in this context implies a mathematical relationship between grams and mole. Think of this as a ratio. The fact that a per relationship, ratio, exists between grams and moles implies that you can use dimensional analysis to interconvert between the two. For example, if we wanted to know the mass of 0.50 mole of molecular hydrogen (H_{2}) we could set up the following equations:
The known molar mass of H_{2} is:
\[\left ( \frac{2.06g\: H_{2}}{1\: mol\: H_{2}} \right )\]
We are given that we have 0.50 moles of H_{2} and we want to find the number of grams of H_{2} that this represents. To perform the dimensional analysis, we arrange the known and the given so that the units cancel, leaving only the units of the item we want to find.
\[(0.5mol\: H_{2})\times \left ( \frac{2.06g\: H_{2}}{1\: mol\: H_{2}} \right )=x\, g\: H_{2}=1.0g\: H_{2}\]
Exercise \(\PageIndex{1}\)
 Determine the mass of 0.752 mol of H_{2} gas.
 How many moles of molecular hydrogen are present in 6.022 grams of H_{2}?
 If you have 22.414 grams of Cl_{2}, how many moles of molecular chlorine do you have?
We can also use what is often called a per relationship (really just a ratio) to convert between number of moles and the number to things (as in 6.02 x 10^{23} things per mole). For example, if we wanted to know how many molecules of H_{2} are there in 3.42 moles of H_{2} gas we could set up the following equations:
The known ratio of molecules per mole is :
\[\left ( \frac{6.02\times 10^{23}molecules\: H_{2}}{1\: mol\: H_{2}} \right )\]
We are given that we have 3.42 moles of H_{2} and we want to find the number of molecules of H_{2} that this represents. To perform the dimensional analysis, we arrange the known and the given so that the units cancel, leaving only the units of the item we want to find.
\[(3.42mol\: H_{2})\times \left ( \frac{6.02\times 10^{23}molecules\: H_{2}}{1\: mol\: H_{2}} \right )=x\: molecules\: H_{2}=2.06\times 10^{24}\: molecules\: H_{2}\]
And finally, we can combine these two operations and use the per relationships to convert between mass and the number of atoms or molecules. For example, if we wanted to know how many molecules of H_{2} are there in 6.022 grams of H_{2} gas we could set up the following series of equations:
The known molar mass of H_{2} is
\[\left ( \frac{2.016gH_{2}}{1molH_{2}} \right )\]
The known ratio of molecules per mole is
\[\left ( \frac{6.02\times 10^{23}molecules\: H_{2}}{1\: mol\: H_{2}} \right )\]
We are given that we have 6.022 grams of H_{2} and we want to find the number of molecules of H_{2} that this represents. As always, to perform the dimensional analysis, we arrange the known ratios and the given so that the units cancel, leaving only the units of the item we want to find.
\[(6.022gH_{2})\times \left ( \frac{1molH_{2}}{2.016gH_{2}}\right )\times \left ( \frac{6.02\times 10^{23}molecules\: H_{2}}{1\: mol\: H_{2}} \right )=x\; molecules\; H_{2}=1.80\times 10^{24}\]
Exercise \(\PageIndex{1}\)
 A sample of molecular chlorine is found to contain 1.0 x 10^{20} molecules of Cl_{2}. What is the mass (in grams) of this sample?
 How many moles of sand, silicon dioxide (SiO_{2}), and how many molecules of sand are found in 1.00 pound (454g) of sand?
 You add 2.64 x 10^{23} molecules of sodium hydroxide (Drano™; NaOH), to your drain. How many moles are this and how many grams?
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