Moles and Formula Mass The Mole 1 dozen

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Moles and Formula Mass

Moles and Formula Mass

The Mole 1 dozen = 12 1 gross = 144 1 ream = 500

The Mole 1 dozen = 12 1 gross = 144 1 ream = 500 1 mole = 6. 022 x 1023 There are exactly 12 grams of carbon-12 in one mole of carbon-12.

Avogadro’s Number 6. 022 x 1023 is called “Avogadro’s Number” in honor of the

Avogadro’s Number 6. 022 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro (1776 -1855). I didn’t discover it. Its just named after me! Amadeo Avogadro

Calculations with Moles: Converting moles to grams How many grams of lithium are in

Calculations with Moles: Converting moles to grams How many grams of lithium are in 3. 50 moles of lithium? 3. 50 mol Li 6. 94 g Li 1 mol Li = 45. 1 g Li

Calculations with Moles: Converting grams to moles How many moles of lithium are in

Calculations with Moles: Converting grams to moles How many moles of lithium are in 18. 2 grams of lithium? 18. 2 g Li 1 mol Li 6. 94 g Li = 2. 62 mol Li

Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 3.

Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 3. 50 moles of lithium? 3. 50 mol 6. 02 x 1023 atoms 1 mol = 2. 07 x 1024 atoms

Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 18.

Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 18. 2 g of lithium? 18. 2 g Li 1 mol Li 6. 94 g Li 6. 022 x 1023 atoms Li 1 mol Li (18. 2)(6. 022 x 1023)/6. 94 = 1. 58 x 1024 atoms Li

Calculating Formula Mass Calculate the formula mass of magnesium carbonate, Mg. CO 3. 24.

Calculating Formula Mass Calculate the formula mass of magnesium carbonate, Mg. CO 3. 24. 31 g + 12. 01 g + 3(16. 00 g) = 84. 32 g

Calculating Percentage Composition Calculate the percentage composition of magnesium carbonate, Mg. CO 3. From

Calculating Percentage Composition Calculate the percentage composition of magnesium carbonate, Mg. CO 3. From previous slide: 24. 31 g + 12. 01 g + 3(16. 00 g) = 84. 32 g 100. 00

Formulas Empirical formula: the lowest whole number ratio of atoms in a compound. Molecular

Formulas Empirical formula: the lowest whole number ratio of atoms in a compound. Molecular formula: the true number of atoms of each element in the formula of a compound. q molecular formula = (empirical formula)n [n = integer] q molecular formula = C 6 H 6 = (CH)6 q empirical formula = CH

Formulas (continued) Formulas for ionic compounds are ALWAYS empirical (lowest whole number ratio). Examples:

Formulas (continued) Formulas for ionic compounds are ALWAYS empirical (lowest whole number ratio). Examples: Na. Cl Mg. Cl 2 Al 2(SO 4)3 K 2 CO 3

Formulas (continued) Formulas for molecular compounds MIGHT be empirical (lowest whole number ratio). Molecular:

Formulas (continued) Formulas for molecular compounds MIGHT be empirical (lowest whole number ratio). Molecular: H 2 O C 6 H 12 O 6 C 12 H 22 O 11 Empirical: H 2 O CH 2 O C 12 H 22 O 11

Empirical Formula Determination 1. Base calculation on 100 grams of compound. 2. Determine moles

Empirical Formula Determination 1. Base calculation on 100 grams of compound. 2. Determine moles of each element in 100 grams of compound. 3. Divide each value of moles by the smallest of the values. 4. Multiply each number by an integer to obtain all whole numbers.

Empirical Formula Determination Adipic acid contains 49. 32% C, 43. 84% O, and 6.

Empirical Formula Determination Adipic acid contains 49. 32% C, 43. 84% O, and 6. 85% H by mass. What is the empirical formula of adipic acid?

Empirical Formula Determination (part 2) Divide each value of moles by the smallest of

Empirical Formula Determination (part 2) Divide each value of moles by the smallest of the values. Carbon: Hydrogen: Oxygen:

Empirical Formula Determination (part 3) Multiply each number by an integer to obtain all

Empirical Formula Determination (part 3) Multiply each number by an integer to obtain all whole numbers. Carbon: 1. 50 x 2 3 Hydrogen: 2. 50 x 2 5 Oxygen: 1. 00 x 2 2 Empirical formula: C 3 H 5 O 2

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H 5 O 2. The molecular mass of adipic acid is 146 g/mol. What is the molecular formula of adipic acid? 1. Find the formula mass of C 3 H 5 O 2 3(12. 01 g) + 5(1. 01) + 2(16. 00) = 73. 08 g

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H 5 O 2. The molecular mass of adipic acid is 146 g/mol. What is the molecular formula of adipic acid? 2. Divide the molecular mass by the mass given by the emipirical formula. 3(12. 01 g) + 5(1. 01) + 2(16. 00) = 73. 08 g

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H

Finding the Molecular Formula The empirical formula for adipic acid is C 3 H 5 O 2. The molecular mass of adipic acid is 146 g/mol. What is the molecular formula of adipic acid? 3. Multiply the empirical formula by this number to get the molecular formula. 3(12. 01 g) + 5(1. 01) + 2(16. 00) = 73. 08 g (C 3 H 5 O 2) x 2 = C 6 H 10 O 4

Conservation of Mass Law In a closed system, the total mass of the system

Conservation of Mass Law In a closed system, the total mass of the system must remain constant. The total mass of the reactants must be equal to the total mass of the products. LAB CONNECTION: This law allowed us to calculate the amount of hydrate in the mixture because the amount of water lost would be uncertain if the starting mass was not the same as the ending mass.

More Conservation Laws à This law implies that matter cannot be created or destroyed.

More Conservation Laws à This law implies that matter cannot be created or destroyed. [Law of conservation of matter] à This is also connected to the Law of Conservation of Atoms, which states that the number of atoms of each type of element on both sides of the equations must be the same.

What happens when a given equation does not conserve mass? # atoms for reactants

What happens when a given equation does not conserve mass? # atoms for reactants ≠ # atoms of products Mass is NOT conserved Must balance the equation by adding coefficients to the elements/compounds in the reaction.

How do we balance equations? For example: Think about a grilled cheese sandwich… 2

How do we balance equations? For example: Think about a grilled cheese sandwich… 2 6

Chemical Equations Chemical change involves a reorganization of the atoms in one or more

Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. C 2 H 5 OH + 3 O 2 ® 2 CO 2 + 3 H 2 O reactants products When the equation is balanced it has quantitative significance: 1 mole of ethanol reacts with 3 moles of oxygen to produce 2 moles of carbon dioxide and 3 moles of water

How do we balance equations? Example Steps __ Zn + _ HCl → __

How do we balance equations? Example Steps __ Zn + _ HCl → __ H 2 + __ Zn. Cl 2 1. Draw a T chart under the equation. Label the left side reactants and the right side products. Write the symbol and number of atoms for each element present in the reaction on its own line on both sides. No, mass is not conserved as the equation is written. 2. Does each element start and end with the same number of atoms? Yes → Mass is conserved and the equation is balanced No → Mass is not conserved and you need to balance the equation. (move on to step 3)

Example Steps __ Zn + 2 HCl → __ H 2 + __ Zn.

Example Steps __ Zn + 2 HCl → __ H 2 + __ Zn. Cl 2 3. If mass is not conserved, you will balance the equation by adding coefficients before molecules. *Do not change any subscripts. * Start with an element that only appears once on each side. On the side that has fewer atoms of that element, add a coefficient before the molecule containing that element, so that the number of atoms of that element on both sides are equal. In the T chart, multiply the coefficient by the subscript on each element in the molecule to get the new numbers of atoms.

Example Steps Final answer: Zn + 2 HCl → H 2 + Zn. Cl

Example Steps Final answer: Zn + 2 HCl → H 2 + Zn. Cl 2 4. Again, does each element start and end with the same number of atoms? Yes → Mass is conserved and the equation is balanced No → Mass is not conserved and you need to change another coefficient. Repeat step 3 Mass is now conserved so the equation is balanced properly.

Calculating Masses of Reactants and Products 1. Balance the equation. 2. Convert mass or

Calculating Masses of Reactants and Products 1. Balance the equation. 2. Convert mass or volume to moles, if necessary. 3. Set up mole ratios. 4. Use mole ratios to calculate moles of desired substituent. 5. Convert moles to mass or volume, if necessary.

Working a Stoichiometry Problem 6. 50 grams of aluminum reacts with an excess of

Working a Stoichiometry Problem 6. 50 grams of aluminum reacts with an excess of oxygen. How many grams of aluminum oxide are formed. 1. Identify reactants and products and write the balanced equation. 4 Al + 3 O 2 2 Al 2 O 3 a. Every reaction needs a yield sign! b. What are the reactants? c. What are the products? d. What are the balanced coefficients?

Working a Stoichiometry Problem 6. 50 grams of aluminum reacts with an excess of

Working a Stoichiometry Problem 6. 50 grams of aluminum reacts with an excess of oxygen. How many grams of aluminum oxide are formed? 4 Al + 3 O 2 2 Al 2 O 3 6. 50 x 2 x 101. 96 ÷ 26. 98 ÷ 4 = 12. 3 g Al 2 O 3 6. 50 g Al 1 mol Al 2 O 3 101. 96 g Al 2 O 3 26. 98 g Al 4 mol Al 1 mol Al 2 O 3 = ? g Al 2 O 3

Limiting Reactant The limiting reactant is the reactant that is consumed first, limiting the

Limiting Reactant The limiting reactant is the reactant that is consumed first, limiting the amounts of products formed.