01/22/2014

Standards: CH3. d. Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.

Objective: Students will be able to practice solving stoichiometry problems through guided and independent practice and complete an assessment with 80% or more accuracy.

Activities: 1. Warm-up

                    2.  Independent Practice – Solving Stoichiometry Problems

                    3.  Assessment- Stoichiometry Quiz

Warm-up

Fe2O3 + 3CO --> 2Fe + 3CO2

In this reaction, how many grams of Fe2O3 are required to

completely react with 84 grams
of CO?

1. A  64 g
2. B  80 g
3. C  160 g
4. D  1400 g 

Standards

CH3. c.Students know one mole equals 6.02 x 10^{23 particles (atoms or molecules).}

CH3. d.Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.

CH3. e.^{Students know how to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products and the relevant atomic masses.}

Learning Objectives

Students will …

1. Calculate the molecular mass and molar mass of a substance.

2. Convert between molecular mass, moles, and molar mass for a substance.

3. Use dimensional analysis to compute the amounts of substances that take part in a chemical reaction.

4. Solve problems in stoichiometry.

Essential Questions

1. Why is the mole used as a unit to measure the amounts of substances?

2. What is special about Avogadro’s number?

Standards:

CH3. c. Students know one mole equals 6.02 x 1023 particles (atoms or molecules).

CH3. d. Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.

CH3. e. Students know how to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products and the relevant atomic masses.

Objective: SWBAT solve stoichiometry problems using the DII Strategy by completing 10 word problems with 80% or more accuracy.

Activities: 1. Warm-up

                   3. DII strategy- 10 Stoichiometry problems

                   4. Assessment - 1 Stoichiometry problem

Warm -up:

How many moles of chlorine gas are contained in 9 02 ×10 . 23 molecules?

A 1.5 moles

B 2.0 moles

C 6.02 moles

D 9.03 moles

Standards:

CH3. c. Students know one mole equals 6.02 x 1023 particles (atoms or molecules).

CH3. d. Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.

CH3. e. Students know how to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products and the relevant atomic masses.

Objective: Students will be able to construct mole ratios from balanced chemical equations and apply these ratios in stoichiometric calculations by means of solving 9 word problems with 88% or more accuracy.

Activities: 1. Warm-up

                   2. Visuals: YouTube video="Stoichiometry"

                   3. DII strategy- 10 Stoichiometry problems

                   4. Assessment - 1 Stoichiometry problem

Warm -up:

How many atoms are in a chromium sample with a mass of 13 grams?

A 1 5. ×1023

B 3 3. ×1023

C 1 9. ×1026

D 2 4×1024

Agenda: Students will be able to balance chemical Equations with 100% accuracy.

Standard:

CH3. c. Students know one mole equals 6.02 x 10²³ particles (atoms or molecules).

CH3. d. Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure.

Objective: Students will be able to solve stoichiometry problems by means of DII strategies with 80 percent or more accuracy.

Activities:1. Warm-up

                 2. DII- practice Stoichiometry problems

                 3. Check for understanding = Student Reflection

Warm-up: How many moles of carbon-12 are contained in exactly 6 grams of carbon-12?

                  A 05mole B 2.0 moles   C 301 ×10²moles    D 602 . ×10²³ moles

Objective: Students will be able to explain what is stochiometry, and interpret balanced chemical equations in terms of moles, representative particles, mass and gas volume at STP.

Activities:1. Warm-up

            2. Visuals: Youtube Video: "Stoichiometry: Chemistry of Massive Creatures

            3. KAGAN Reading: ch 12.1 "The Arithmetic of Equations.

           4. DII practice: Stoichiometry worksheet

Homework: page 358: Conceptual problems 12.1 

12/12/2013- Chemistry

Objective: Students will convert moles to grams and grams to

                     Moles with 80% accuracy.

Activities: 1. Warm-up

                   2. DII-practice: Moles Worksheet

                   3. Check for understanding

Warm-up: How many atoms are in H₂SO₄?