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Posted: April 10th, 2022
stoichiometry
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.
1. A sample of gold (Au) has a mass of 35.12 g. 
molar mass
a. 
Calculate 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.
2. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.
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.
Then, add all 3 totals to find total molar mass of C12H22O11.
Then calculate moles of C12H22O11.
b. 
Calculate 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.
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.)
|
| 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 |
|
|
|
|
|||||
| Question #2 |
|
|
|
|
|
|||||
| Data Table |
|
|
|
|
|
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.
1. A sample of gold (Au) has a mass of 35.12 g. molar mass
a. Calculate 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.
2. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.
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.
Then, add all 3 totals to find total molar mass of C12H22O11.
Then calculate moles of C12H22O11.
b. Calculate 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.
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.)
|
| 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 |
|
|
|
|
|||||
| Question #2 |
|
|
|
|
|
|||||
| Data Table |
|
|
|
|
|
Total points: ___ /20
Comments :
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