READ: Conversions Between Moles and Mass

READ: Conversions Between Moles and Mass

The molar mass of any substance is the mass in grams of one mole of representative particles of that substance.  The representative particles can be atoms, molecules, or formula units of ionic compounds.  This relationship is frequently used in the laboratory.  Suppose that for a certain experiment you need 3.00 moles of calcium chloride (CaCl₂).  Since calcium chloride is a solid, it would be convenient to use a balance to measure the mass that is needed.  The molar mass of CaCl₂ is 110.98 g/mol.  The conversion factor that can be used is then based on the equality that 1 mol = 110.98 g CaCl₂.  Dimensional analysis will allow you to calculate the mass of CaCl₂ that you should measure.

3.00 mol CaCl2×110.98 g CaCl21 mol CaCl2=333 g CaCl2

When you measure the mass of 333 g of CaCl₂, you are measuring 3.00 moles of CaCl₂.

Sample Problem: Converting Moles to Mass

Chromium metal is used for decorative electroplating of car bumpers and other surfaces.  Find the mass of 0.560 moles of chromium.

Step 1: List the known quantities and plan the problem.

Known

• molar mass of Cr = 52.00 g mol
• 0.560 mol Cr

Unknown

• 0.560 mol Cr = ? g

One conversion factor will allow us to convert from the moles of Cr to mass.

Step 2: Calculate.

0.560 mol Cr×52.00 g Cr1 mol Cr=29.1 g Cr

Step 3: Think about your result.

Since the desired amount was slightly more than one half of a mole, the mass should be slightly more than one half of the molar mass.  The answer has three significant figures because of the 0.560 mol.

A similar conversion factor utilizing molar mass can be used to convert from the mass of an substance to moles.  In a laboratory situation, you may perform a reaction and produce a certain amount of a product which can be massed.  It will often then be necessary to determine the number of moles of the product that was formed.  The next problem illustrates this situation.

Sample Problem: Converting Mass to Moles

A certain reaction produces 2.81 g of copper(II) hydroxide, Cu(OH)₂.  Determine the number of moles produced in the reaction.

Step 1: List the known quantities and plan the problem.

Known

• mass = 2.81 g

Unknown

• mol Cu(OH)₂

One conversion factor will allow us to convert from mass to moles.

Step 2: Calculate.

First, it is necessary to calculate the molar mass of Cu(OH)₂ from the molar masses of Cu, O, and H.  The molar mass is 97.57 g/mol.

2.81 g Cu(OH)2×1  mol Cu(OH)297.57 g Cu(OH)2=0.0288 mol Cu(OH)2

Step 3: Think about your result.

The relatively small mass of product formed results in a small number of moles.

Summary

• Calculations involving conversions between moles of a material and the mass of that material are described.

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