Unit 6 Lesson 3 Activity: Stoichiometry

 

 

 

CHEMISTRY

 

 

 

 

 

Stoichiometry can be thought of as the math of chemistry. It involves using relationships between reactants and/or products to determine such quantities as mass, moles, and number of atoms. Dimensional analysis is a way to simplify stoichiometric problem solving. In this activity, you will use dimensional analysis in order to count the number of atoms in a given substance.

 

 

 

 

 

Text Box: Record in Table 11.  A sample of gold (Au) has a mass of 35.12 g.                            http://www.chemistryexplained.com/images/chfa_02_img0374.jpgmolar mass

 

a.   Text Box: Record in Table 1Calculate the number of moles of gold (Au) in the sample and record in Table 1. Show your work below.

 

b.   Calculate the number of atoms of gold (Au) in the sample and record in Table 1. Show your work below.

 

 

 

 

 

 

Text Box: Record in Table 1

 

 

 

2.  A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.

 

oxygenhttp://www.chemteam.info/Mole/Hydrogen.GIF

 

a.   Calculate the number of moles of C12H22O11 contained in the sample and record in Table 1. Show your work. (Start with molar mass from periodic table and multiply by number of atoms of each element.)

 

a.    Find molar mass of Carbon. .         1.202 g (1mol sucrose)/(342g)=3.5 x 10^-3 mol surcose

 

 

 

 

Find molar mass of Hydrogen.

 

 

Find molar mass of Oxygen.

 

 

 

 

Text Box: Record in Table 1Then, add all 3 totals to find total molar mass of C12H22O11.

 

Then calculate moles of C12H22O11.

 

 

b.   Text Box: Record in Table 1Calculate the moles of each element in C12H22O11 and record in Table 1. Show your work. Take the moles of C12H22O11 and multiply by the number of atoms of each element in the compound.

 

 

Text Box: Record in Table 1Text Box: Record in Table 1

 

 

c.    Calculate the number of atoms of each type in C12H22O11 record in Table 1. Show your work. Take the moles of each element above and multiply by 6.02 x 1023 to find the number of atoms of each element in the compound. Make sure your answers are correctly written in scientific notation (In scientific notation all numbers are expressed as a product of a number that is > 1 but < 10  and an exponent of 10.)

 

 

 

 

Text Box: Record in Table 1

 

 

 

Text Box: Record in Table 1

 

 

Text Box: Record in Table 1

 

 

 

 

Table 1

 
 

 

Au

C12H22O11
Mass (grams)

35.12 g

 

1.202 g
Molar mass (g/mol)  

 

  
 

 

 

 

 

Moles of each element

  

 

 

 

Au moles:

  

C:

 

 

H:

 

 

O:

 
 

 

 

Atoms of each element

 

 

 

  

 

Atoms of Au:

  

C:

 

 

H:

 

 

O:

 

 

 

 

 

 

 

 

 

 

 

 

 

 

RUBRIC

 

 

 

 

3

2

1

0

Points Awarded
Question #1 N/A  

Work is shown for both calculations.

 

  

 Work is shown for one calculation.

 

  

 Work is not shown for any calculation.

 

  

                ___ /2

 
Question #2  

 All work is shown for three calculations.

 

  

 All work is shown for both calculations.

 

  

 All work is shown for one calculation.

 

  

 Work is not shown for any calculation.

 

  

 ___×3 = ___ /9

 
Data Table  

 All data is accurate.

 

  

 Most data is accurate.

 

  

 Little data is accurate.

 

  

 No data is accurate.

 

  

 ___×3 = ___ /9

 

 

 

 

Total points: ___ /20

 

Comments :

 

 

 

 

 

Name:                                                                            Date:

 

 

 

   

 

Unit 6 Lesson 3 Activity: Stoichiometry

 

 

 

CHEMISTRY

 

 

 

 

 

Stoichiometry can be thought of as the math of chemistry. It involves using relationships between reactants and/or products to determine such quantities as mass, moles, and number of atoms. Dimensional analysis is a way to simplify stoichiometric problem solving. In this activity, you will use dimensional analysis in order to count the number of atoms in a given substance.

 

 

 

 

 

Text Box: Record in Table 11.  A sample of gold (Au) has a mass of 35.12 g.                            http://www.chemistryexplained.com/images/chfa_02_img0374.jpgmolar mass

 

a.   Text Box: Record in Table 1Calculate the number of moles of gold (Au) in the sample and record in Table 1. Show your work below.

 

b.   Calculate the number of atoms of gold (Au) in the sample and record in Table 1. Show your work below.

 

 

 

 

 

 

Text Box: Record in Table 1

 

 

 

2.  A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.

 

oxygenhttp://www.chemteam.info/Mole/Hydrogen.GIF

 

a.   Calculate the number of moles of C12H22O11 contained in the sample and record in Table 1. Show your work. (Start with molar mass from periodic table and multiply by number of atoms of each element.)

 

a.    Find molar mass of Carbon. .         1.202 g (1mol sucrose)/(342g)=3.5 x 10^-3 mol surcose

 

 

 

 

Find molar mass of Hydrogen.

 

 

Find molar mass of Oxygen.

 

 

 

 

Text Box: Record in Table 1Then, add all 3 totals to find total molar mass of C12H22O11.

 

Then calculate moles of C12H22O11.

 

 

b.   Text Box: Record in Table 1Calculate the moles of each element in C12H22O11 and record in Table 1. Show your work. Take the moles of C12H22O11 and multiply by the number of atoms of each element in the compound.

 

 

Text Box: Record in Table 1Text Box: Record in Table 1

 

 

c.    Calculate the number of atoms of each type in C12H22O11 record in Table 1. Show your work. Take the moles of each element above and multiply by 6.02 x 1023 to find the number of atoms of each element in the compound. Make sure your answers are correctly written in scientific notation (In scientific notation all numbers are expressed as a product of a number that is > 1 but < 10  and an exponent of 10.)

 

 

 

 

Text Box: Record in Table 1

 

 

 

Text Box: Record in Table 1

 

 

Text Box: Record in Table 1

 

 

 

 

Table 1

 
 

 

Au

C12H22O11
Mass (grams)

35.12 g

 

1.202 g
Molar mass (g/mol)  

 

  
 

 

 

 

 

Moles of each element

  

 

 

 

Au moles:

  

C:

 

 

H:

 

 

O:

 
 

 

 

Atoms of each element

 

 

 

  

 

Atoms of Au:

  

C:

 

 

H:

 

 

O:

 

 

 

 

 

 

 

 

 

 

 

 

 

 

RUBRIC

 

 

 

 

3

2

1

0

Points Awarded
Question #1 N/A  

Work is shown for both calculations.

 

  

 Work is shown for one calculation.

 

  

 Work is not shown for any calculation.

 

  

                ___ /2

 
Question #2  

 All work is shown for three calculations.

 

  

 All work is shown for both calculations.

 

  

 All work is shown for one calculation.

 

  

 Work is not shown for any calculation.

 

  

 ___×3 = ___ /9

 
Data Table  

 All data is accurate.

 

  

 Most data is accurate.

 

  

 Little data is accurate.

 

  

 No data is accurate.

 

  

 ___×3 = ___ /9

 

 

 

 

Total points: ___ /20

 

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