23/10: Reacting masses

• Chemistry
• Secondary Education

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CHEMISTRY 10

                   20: Reacting masses

Week 11

Good Afternoon!

• Where will you put your learning materials: notebook, workbook, coursebook, pen and pencil, and laptop?
  
• Have you kept your phone in your locker?
• Have you joined our LessonUp slides?
• Have you gone to the bathroom before the class starts?
• Have you checked any announcements or missing work on our Google Classroom?
• Are you seated in your assigned chair?

10S1_Classwork 9: Stoichiometry (part 2)

Apply your learned knowledge and skills:

Choose one. (2 marks)

Write the word and balanced symbol equations.

Option 1: When added to dilute hydrochloric acid, copper (II) carbonate fizzes and releases carbon dioxide gas. The resulting solution is copper (II) chloride and water.

Option 2: Magnesium carbonate fizzes and releases carbon dioxide gas when added to dilute sulfuric acid. The resulting solution is magnesium sulfate and water.

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CHEMISTRY 10

                   20: Reacting masses

Week 11

calculate the Aᵣ or Mᵣ of atoms and molecules/ ions.

calculate reacting masses in simple proportions.

assess my thinking and how I learn to identify growth areas and improve my learning.

What mass of carbon dioxide would be produced if 6 g of carbon was completely combusted?

What mass of carbon dioxide would be produced if 6 g of carbon was completely combusted (burned)?

C + O₂ → CO₂

What mass of carbon dioxide would be produced if 6 g of carbon was completely combusted (burned)?

C + O₂ → CO₂

Let's review the Aᵣ or Mᵣ .

I can calculate the Aᵣ or Mᵣ of atoms and molecules/ ions.

Yes, I can confidently do it.

Yes, I can but need more practice.

No, I lack confidence so I need more practice or ask help from my teacher.

Chemists often need to know how much of a substance has been formed or used up during a chemical reaction. Why?

• In the chemical industry, the substances being reacted (the reactants) and the substances being produced (the products) are worth thousands of dollars!

Chemists often need to know how much of a substance has been formed or used up during a chemical reaction. Why?

• In the chemical industry, the substances being reacted (the reactants) and the substances being produced (the products) are worth thousands of dollars!

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CHEMISTRY 10

                   20: Reacting masses

Week 11

What mass of carbon dioxide would be produced if 6 g of carbon was completely combusted?

C + O₂ → CO₂

STEPS YOU CAN FOLLOW:

• Write a balanced symbol equation for the given reaction.
• Work out the relative formula mass of molecules.
• Use the symbol equation.
• Convert these relative masses to actual masses by adding mass units, g.
• Relate the masses.

Sample 1

What mass of carbon dioxide would be produced if 6 g of carbon was completely combusted?

So, 6 g of burning carbon would result in the formation of how much carbon dioxide gas is in grams?

STEPS YOU CAN FOLLOW:

• Write a balanced symbol equation for the given reaction.
• Work out the relative formula mass of molecules.
• Use the symbol equation.
• Convert these relative masses to actual masses by adding mass units, g.
• Relate the masses.

Sample 1

What mass of hydrogen gas would be produced if 46 g of sodium was reacted with water?

STEPS YOU CAN FOLLOW:

• Write a balanced symbol equation for the given reaction.
• Work out the relative formula mass of molecules.
• Use the symbol equation.
• Convert these relative masses to actual masses by adding mass units, g.
• Relate the masses.

Sample 2

I can calculate reacting masses in simple proportions.

Yes, I can confidently do it.

Yes, I can but need more practice.

No, I lack confidence so I need more practice or ask help from my teacher.

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CHEMISTRY 10

                   20: Reacting masses

Week 11

PRACTICE WORK

Pair up. Choose ONE only.

• What mass of carbon dioxide gas would be produced if 10 g of calcium carbonate reacted with an excess of hydrochloric acid?

• What mass of sulfur dioxide would be produced if 64 tonnes of sulfur were completely reacted with oxygen gas? (1 tonne = 1000 kg)

Sample 3

Share your thought process.

I can calculate reacting masses in simple proportions.

Yes, I can confidently do it.

Yes, I can but need more practice.

No, I lack confidence so I need more practice or ask help from my teacher.

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CHEMISTRY 10

                   20: Reacting masses

Week 11

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STEM Project

Building a Futuristic City Scale Model

Week 11

Share your thought process.