How can molar mass be used as a conversion factor

Find the mass of each of the products formed. Prepare two concept maps and use the proper conversion factor.

The balanced chemical equation is as follows. How many grams of HCl are produced by the reaction of Learning Objectives Perform conversions between mass and moles of a substance. Convert from mass or moles of one substance to mass or moles of another substance in a chemical reaction. Use a balanced chemical equation to determine molar relationships between substances. Molar Mass The molar mass of any substance is the mass in grams of one mole of representative particles of that substance.

Solution Steps for Problem Solving Calculate the mass of 3. Identify the "given"information and what the problem is asking you to "find. Cancel units and calculate. The calculated value makes sense because it is almost four times times the mass for 1 mole of aluminum.

Our final answer is expressed to four significant figures. Answer 3. Answer: Solution Steps for Problem Solving How many moles are present in grams of water? Answer: g. Mole and Mass Relationships in Chemical Equations We have established that a balanced chemical equation is balanced in terms of moles as well as atoms or molecules.

Since g of AlCl 3 is less than Molar Relationships in Chemical Equations Previously, you learned to balance chemical equations by comparing the numbers of each type of atom in the reactants and products. Solution Steps for Problem Solving How many moles of oxygen react with hydrogen to produce Think about your result. Since each mole of oxygen produces twice as many moles of water, it makes sense that the produced amount is greater than the reactant amount.

Solution Steps for Problem Solving How many moles of ammonia are produced if 4. The result corresponds to the ratio of hydrogen to ammonia from the balanced equation. The mole is the universal measurement of quantity in chemistry. However, the measurements that researchers take every day provide answers not in moles but in more physically concrete units, such as grams or milliliters.

Therefore, scientists need some way of comparing what can be physically measured to the amount of measurement they are interested in: moles. Because scientists of the early 18th and 19th centuries could not determine the exact masses of the elements due to technology limitations, they instead assigned relative weights to each element. From this scale, hydrogen has an atomic weight of 1. Chemists generally use the mole as the unit for the number of atoms or molecules of a material.

One mole abbreviated mol is equal to 6. The molar mass of any element can be determined by finding the atomic mass of the element on the periodic table.

For example, if the atomic mass of sulfer S is To see why these elements have different molar masses, we need to remember that the atoms of different elements contain different numbers of protons, neutrons, and electrons, so they have different masses. The atomic masses given in the periodic table inside the front cover of this book represent the different weighted average masses of the naturally occurring atoms of each element. Different atomic masses lead to different molar masses.

For example, the atomic mass of magnesium Thus the molar mass of magnesium is