# Mole to relationship ppt

5 The Law of Conservation of Mass In a chemical reaction, matter is never created or destroyed. The number of atoms and the mass of the reactants must be. Outline The Mole and Avogadro's Number Gram-Mole Conversions Mole Relationships and Chemical Equations Mass Relationships and Chemical. The mole (mol) is a unit of measure for an amount of a chemical substance. We can use the mole relationship to convert between the number of particles and.

Using mole ratios, calculate the mass of product that can be formed from a given mass of reactant.

## Mole relationships in chemical equations

Actual amounts of substances used in the laboratory are weighed out in grams. Three types of conversions are needed when doing chemical arithmetic. Write the balanced chemical equation.

Choose molar masses and mole ratios to convert the known information into the needed information. Set up the factor-label expression. Calculate the answer and check the answer against the ballpark estimate you made before you began your calculations. The molecular weight of HNO3 is We are given the number of moles of a reactant and are asked to find the mass of a product.

Problems of this sort always require working in moles and then converting to mass. We need a mole to mole conversion to find the number of moles of product, and then a mole to mass conversion to find the mass of product. For the first conversion, we use the mole ratio of HNO3 to NO2 as a conversion factor, and for the mole to mass calculation, we use the molar mass of HNO3 Set up factor labels.

Mole Ratio Practice Problems

What mass of calcium chloride was used as reactant? Both the known information and that to be found are masses, so this is a mass-to-mass conversion problem. The mass of CaC2O4 is first converted into moles, a mole ratio is used to find moles of CaCl2, and the number of moles of CaCl2 is converted into mass. We will need three conversion factors.

• Mole-Mass and Mole-Volume Relationships
• Ch Mole-Mass and Mole-Volume Relationship

We will need to perform gram to mole and mole to mole conversions to get from grams CaC2O4 to grams CaCl2. Using mole ratios and the mass of reactants, calculate the theoretical yield and percent yield for a reaction. The limiting reagent is the reactant that runs out first.

### PPT - The Mole–Mass Relationship PowerPoint Presentation - ID

Chemical reactions do not always yield the exact amount predicted. Actual yield is the amount of product actually formed in a reaction. Calculate the percent yield for this reaction if the actual yield is only The percent yield is calculated by dividing the actual yield by the theoretical yield and multiplying by The molar masses of boric oxide and magnesium are To calculate theoretical yield, we first have to identify the limiting reagent.

The theoretical yield in grams is then calculated from the amount of limiting reagent used in the reaction.

We have the masses and molar masses of the reagents g B2O3, molar mass We are solving for the theoretical yield of boron. We can use the molar masses to convert from masses to moles of reactants B2O3, Mg.

From moles of reactants, we can use mole ratios from the balanced chemical equation to find the number of moles of B produced, assuming complete conversion of a given reactant. B2O3 is the limiting reagent, since complete conversion of this reagent yields less product Once the limiting reagent has been identified B2O3the theoretical amount of B that should be formed can be calculated using a mole to mass conversion. Never change any subscripts in a formula 3.

Coefficients should be written as the lowest possible ratios 4.

What if I wanted tricycles? Balanced chemical equations can be used to calculate how much reactant we will use or how much product is formed from a chemical reaction 25 Coefficients indicate relative numbers of moles or molecules of reactants and products. One molecule of hydrogen gas reacts with one molecule of chlorine gas to yield two molecules of hydrogen chloride gas. How many moles of carbon dioxide? How many moles of water vapor?

How many moles of sodium hydrogen carbonate? How many moles of oxygen gas? How many moles of hydrogen gas? Mole ratio of water to hydrogen gas.