Introduction to Stoichiometry

​Balancing Equations Video

Multiple Choice

Balance this equation-
__P₄ + __O₂ --> __P₂O₃

• it is already balanced
• 2, 1, 3
• 1, 2, 3
• 1, 3, 2

Multiple Choice

Balance this equation.

__CH₄ + __O₂ --> __CO₂ + __H₂O

• 1,2,1,1

• 2,1,2,1

• 1,2,1,2

• 0,2,0,2

Fill in the Blanks

Indicate the respective coefficients needed to balance the chemical equation.

SiCl₄(s) + H₂O(l) → H₄SiO₄(s) + HCl(l)

Fill in the Blanks

Indicate the respective coefficients needed to balance the chemical equation.

NO₂(g) + H₂O(l) → HNO₃(aq) + NO(g)

Drag and Drop

Create a word equation from the description of the given reaction: Solid silver reacts with aqueous nitric acid to produce aqueous silver nitrate, liquid water, and gaseous nitrogen monoxide.



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Placeholder

(s) + ​

Placeholder

(aq) → ​

Placeholder

(aq) + ​

Placeholder

(l) + ​

Placeholder

(g)

Drag these tiles and drop them in the correct blank above

silver

nitric acid

silver nitrate

water

nitrogen monoxide

solid

aqueous

liquid

gas

aqueous solution

Fill in the Blanks

What is the chemical formula for nitric acid?

Fill in the Blanks

What is the chemical formula for silver nitrate?

Fill in the Blanks

What is the chemical formula for nitrogen monoxide?

Fill in the Blanks

Indicate the respective coefficients needed to balance the chemical equation.

$Ag\left(s\right)\ +\ HNO_3\left(aq\right)\ \rightarrow\ AgNO_3\left(aq\right)\ +\ H_2O\left(l\right)\ +\ NO\left(g\right)$

Drag and Drop

Create a word equation from the description of the given reaction: Shiny copper metal forms from a blue solution of copper(II) sulfate when a new iron nail is immersed in it, leaving behind a pale green iron(II) sulfate solution.



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Placeholder

(s) + ​

Placeholder

(aq) → ​

Placeholder

(aq) + ​

Placeholder

(s)

Drag these tiles and drop them in the correct blank above

iron

copper(II) sulfate

iron(II) sulfate

copper

green

blue

shiny

reactant

product

Fill in the Blanks

Indicate the respective coefficients needed to balance the chemical equation.

iron(s) + copper(II) sulfate(aq) → iron(II) sulfate(aq) + copper(s)

Calculating Molar Mass

Converting with Molar Mass

Multiple Choice

Calculate the molar mass of NaHCO₃.

• 84.01 g/mol

• 86.98 g/mol

• 87.56 g/mol

• 84.0 g/mol

Multiple Choice

Calculate the molar mass of Ca₃(PO₄)₂.

• 310.18 g/mol

• 135.05 g/mol

• 279.21 g/mol

• 342.18 g/mol

Fill in the Blanks

What is the molar mass of chlorine?

Fill in the Blanks

Calculate the molar mass of barium acetate, Ba(C₂H₃O₂)₂

Labeling

How many moles are in a 12.83 g sample of Iron(III) sulfate?

Drag the terms into the proper spot to set up the problem to solve this question.

Drag labels to their correct position on the image

1 mol Fe₂(SO₄)₃

1

399.91 g Fe₂(SO₄)₃

12.83 g Fe₂(SO₄)₃

Fill in the Blanks

How many moles are in a 12.83 g sample of Iron(III) sulfate?

Labeling

How many grams are in 7.96 moles of calcium chloride?

Drag the terms into the proper spot to set up the problem to solve this question.

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1 mol CaCl₂

1

7.96 mol CaCl₂

110.98 g CaCl₂

Fill in the Blanks

How many grams are in 7.96 moles of calcium chloride?

Fill in the Blanks

How many moles of sodium chloride are in a 321.8 g sample?

Fill in the Blanks

A sample containing 0.829 moles of cobalt contains how many grams of cobalt?

​Mole Ratios

Labeling

3 Ag(s) + 4 HNO₃(aq) → 3 AgNO₃(aq) + 2 H₂O(l) + NO(g)

How many moles of silver are needed to react with 40. moles of nitric acid?

Drag and drop to set up the problem.

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40. mol HNO₃

3 mol Ag

4 mol HNO₃

1

Multiple Choice

3 Ag(s) + 4 HNO₃(aq) → 3 AgNO₃(aq) + 2 H₂O(l) + NO(g)

How many moles of silver are needed to react with 40. moles of nitric acid?

• 30. mol Ag

• 0.33 mol Ag

• 0.19 mol Ag

• 53 mol Ag

Labeling

N₂H₄(l) + N₂O₄(l) → N₂(g) + H₂O(g)

How many moles of dinitrogen tetrahydride are required to produce 57 moles of nitrogen?

Drag and drop to set up the problem.

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1 mol N₂O₄

3 mol N₂

57 mol N₂O₄

1

1 mol N₂

4 mol N₂H₄

57 mol N₂

1 mol N₂H₄

Multiple Choice

N₂H₄(l) + N₂O₄(l) → N₂(g) + H₂O(g)

How many moles of dinitrogen tetrahydride are required to produce 57 moles of nitrogen?

• 38 mol N₂H₄

• 86 mol N₂H₄

• 0.026 mol N₂H₄

• 0.012 mol N₂H₄

Multiple Choice

$$16Na\left(s\right)\ +\ S_8\ \left(s\right)\ \rightarrow\ 8Na_2S\ \left(s\right)$$

What is the total number of moles of sulfur that reacts when 4.0 moles of sodium were completely consumed?

• 1.0

• 0.25

• 0.50

• 16

Drag and Drop

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.



Remember that every stoichiometry problem requires a balanced chemical equation.



Drag and drop the terms to create the word equation for the chemical reaction.



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Placeholder

(s) +​

Placeholder

(g) →​

Placeholder

(s)

Drag these tiles and drop them in the correct blank above

aluminum

oxygen

aluminum oxide

mass

moles

reactants

synthesis

products

Fill in the Blanks

What is the chemical formula for aluminum oxide?

Multiple Choice

What type of reaction is given for this problem?

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

• combustion

• decomposition

• double replacement

• single replacement

• synthesis

Multiple Choice

What are the coefficients that will balance the equation?

$$Al\left(s\right)\ +\ O_2\left(g\right)\ \rightarrow\ Al_2O_3\left(s\right)$$

• 1, 1, 1

• 4, 3, 2

• 2, 1, 1

• 2, 3, 2

Multiple Choice

What is the FIND for the problem?

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

• g Al₂O₃

• mol Al

• g Al

• mol Al₂O₃

Fill in the Blanks

What is the starting point for your calculation (the Given)?

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

Reorder

Arrange the following in order needed to solve the problem.

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

• Write a balanced chemical equation

• Convert moles Al to moles Al₂O₃

• Convert moles Al₂O₃ to grams Al₂O₃

1

2

3

• 1
• 2
• 3

Labeling

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

Drag and drop to set up the problem.

Drag labels to their correct position on the image

3 mol O₂

1 mol Al₂O₃

103.96 g Al₂O₃

1

3.75 mol Al

4 mol Al

2 mol Al₂O₃

32.00 g O₂

27.98 g Al

Multiple Choice

Calculate the mass of aluminum oxide produced when 3.75 moles of aluminum burn in oxygen.

• 195 g Al₂O₃

• 780. g Al₂O₃

• 0.0180 g Al₂O₃

• 55.4 g Al₂O₃

Multiple Choice

At extremely high temperatures, solid manganese metal is produced along with a white, powdery aluminum oxide, when aluminum powder reacts with a solid manganomanganic oxide ore that has a chemical formula of Mn₃O₄.

What are the coefficients for the reaction? (Hint: write a word equation first.)

• 1, 1, 1, 1

• 3, 8, 4, 9

• 1, 2, 1, 4

• 6, 10, 9, 7

Fill in the Blanks

At extremely high temperatures, solid manganese metal is produced along with a white, powdery aluminum oxide, when aluminum powder reacts with a solid manganomanganic oxide ore that has a chemical formula of Mn₃O₄. How many moles of aluminum oxide are made if 3580 g of manganomanganic oxide are consumed?