This document provides information about performing calculations using balanced chemical equations. It discusses the three main types of calculations: (1) mole-to-mole conversions using mole ratios from balanced equations, (2) mole-to-mass conversions using molar masses, and (3) mass-to-mass conversions that involve multiple steps. Sample problems are provided as examples for each type of calculation. Key steps like identifying the problem, finding the appropriate conversion factor, and using dimensional analysis are emphasized.

1. Calculations with
Balanced Equations
Q1_WEEK 6

2. Learning Target:
1. mole or mass ratios for a reaction in
order to calculate the amount or
reactant needed or amount of product
formed in terms of moles or mass,
(STEM_GC11MRlg-h-38).

3. What I know?

4. Group 1: 16pcs

5. Group 2: 24pcs

6. Group 3: 32pcs

7. Group 1: 40pcs

8. Calculations with Balanced Equations

9. What's in?
LET US HAVE SOME FUN!
CRYPTOGRAM - Identify the
mystery word by
deciphering the given
code and knowing the
clue.

10. What's New?
2. Mass
IMPORTANT VOCABULARY WORDS
Vocabulary Word Meaning
1. Mole Amount of any substance that contains.
The amount of matter possessed by an object.
Avogadro's number of particles (6.02 X 1023 atoms).

11. What is it?
Conservation of Matter
The law of conservation of matter, also known as the
conservation of mass, states that the amount of matter in
a closed system never changes. Meaning, the amount of
matter before and after the reaction are always equal.

12. What are the Calculations Involved in a
Balanced Equations?
(1) Mole-to-Mole Conversion,
(2) Moles-to-Mass Conversion and
(3) Mass-to-Mass Calculation.

13. If the number of moles of one substance is
given in the problem, we can determine the
number of moles of any of the other substances in
the chemical reaction or chemical equation by
using a mole conversion factor based on the
coefficients in the balanced chemical equation.
1. Mole-to-Mole Conversion

14. Important Steps in Mole-to-Mole Conversion
4NH3 + 3O2 2N2 + 6H2O
How many moles of O2 are needed to react with 8
moles of NH3?

15. Step 1. Analyze the given chemical equation.
In the given chemical equation, there are;
No. of Mole Substance
4 NH3
3 O2
2 N2
6 H2O
Step 2. Identify the problem.
_ ?__ moles of O2 : 8 moles of NH3?
4NH3 + 3O2 2N2 + 6H2O

16. Step 3. Identify the conversion factor based from the balanced
chemical equation.
Based from the given chemical equation, there are 3 moles of
for every 4 moles of NH3. Therefore, the conversion factor would be;
3 mole O2 or 4 mole NH3
4 mole NH3 3 mole O2
Step 4. Dimensional Analysis using the identified conversion factor.
8 mole NH3 x 3 mole O2__ = 6 mole O2
4 mole NH3
4NH3 + 3O2 2N2 + 6H2O

18. The gram is the most convenient unit for
measuring amounts of reactants or products in the
laboratory. In order to convert moles to grams or
grams to moles, you have to make use of the molar
mass of the given compound.
2. Mole-to-Mass Conversion

19. Important Steps in Mole-to-Mole
Conversion
4NH3 + 3O2 2N2 + 6H2O
How many grams of O2 are needed to react with 10
moles of NH3?

20. Step 1. Identify the problem.
_?_grams of O2 : 10 moles of NH3?
Step 2. Identify the conversion factor based from the balanced
chemical equation.
Based from the given chemical equation, there are 3
moles of O2 for every 4 moles of NH3. Therefore, the
conversion factor would be;
3 mole O2 or 4 mole NH3
4 mole NH3 3 mole O2
4NH3 + 3O2 2N2 + 6H2O

21. Step 3. Find out the number of moles of O2 needed to react to 10 moles NH3
using the Dimensional Analysis.
10 mole NH3 X _3 mole O2__ = 7.5 mole O2
4mole NH3
Step 4. Change the moles of O2 to grams using the molar mass of O2 as
conversion factor. The molar mass of O2 is 32.0 g because each O has a mass
number of 16.
7.5 mole O2 x _32.0 g O2__ = 240.0 g O2
1 mole O2
4NH3 + 3O2 2N2 + 6H2O

23. If the problem asks for the mass in grams of one
substance and the mass of another substance is
given.
3. Mass-to-Mass Conversion

24. Steps in Mass-to-Mass Conversion
2C2H6 + 7O2 4CO2 + 6H2O
How many grams of O2 are needed to react with 250g
of 2C2H6?

25. Step 1. Identify the problem.
? grams of O2 : 250 grams of 2C2H6?
Step 2. Change the grams of 2C2H6 to moles of 2C2H6.
The molar mass of C2H6 is 30.0 g because the mass number
of C is 12 multiply by 2 and that would be 24.0 g while the mass
number of H is 1 multiply by 6 and that would be 6.0 g. So, the
total molar of C2H6 is 30.0 g.
250g C2H6 x 1 mole C2H6_ = 8.33 mole C2H6
30.0 g C2H6
2C2H6 + 7O2 4CO2 + 6H2O

26. Step 3. Change moles of C2H6 to moles of O2
8.33 mole C2H6 x _7 mole O2_ = 29.2 mole O2
2 mole C2H6
Step 4. Change the moles of O2 to grams of O2.
29.2 mole O2 x _32g O2___ = 934.0g O2
1 mole O2
Therefore, the amount of oxygen needed is 934.0 grams.
2C2H6 + 7O2 4CO2 + 6H2O

27. PRACTICE EXERCISE : Problem Solving How many grams of H2 are
needed to react with 4.5 moles of N2?
N2 + 3H2 2NH3
Step 1. Identify the problem.
Step 2. Identify the conversion factor based from the
balanced chemical equation.
Step 3. Find out the number of moles using the Dimensional
Analysis.
Step 4. Change the moles using the molar mass.

28. Activity 2 – FREEDOM WALL
Procedure:
1. Given set of problems, choose 1 that you want to present. You
need to follow the steps in solving the problem.
2. You may add design that you want or remark as your
expression of your feelings or experiences towards the solving
process.
3. Post your output on TEAMS Assignment.
Performance Task No. 5

29. SET OF CHEMICAL FORMULAS
1. The combustion of propane C3H8, a fuel used in background grills and camp stoves,
produces carbon dioxide and water vapor. How many moles of carbon dioxide are formed
from 5.60 moles of propane?
2. Solid xenon hexafluoride is prepared by allowing xenon gas and fluorine gas to react. If
50.0g of xenon are consumed in the reaction, how many grams of xenon hexafluoride are
formed?
Output Presentation

30. Go to TEAMS Assignment and answer
Assessment No. 6
Assessment No. 6

31. Thank You!