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

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.



​

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

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.



​

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

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

Labelling

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

12.83 g Fe₂(SO₄)₃

1 mol Fe₂(SO₄)₃

399.91 g Fe₂(SO₄)₃

1

Labelling

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

7.96 mol CaCl₂

1

110.98 g CaCl₂

​Mole Ratios

Labelling

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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4 mol HNO₃

1

40. mol HNO₃

3 mol Ag

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

Labelling

N₂H₄(l) + N₂O₄(l) → N₂(g) + H₂O(g)

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

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1 mol N₂O₄

57 mol N₂O₄

1 mol N₂

1 mol N₂H₄

57 mol N₂

1

3 mol N₂

4 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.



​

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

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

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

Labelling

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

27.98 g Al

32.00 g O₂

4 mol Al

2 mol Al₂O₃

3 mol O₂

103.96 g Al₂O₃

3.75 mol Al

1 mol Al₂O₃

1

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