Lesson: Conservation of Mass Glencoe Science • Chemistry • Concepts and Applications • Glencoe • Chemistry • Matter & Change • Basic Chemistry • Sixth Edition • Glencoe Science • Chemistry • Chemical Interactions • Chemistry • The Molecular Nature of Matter and Change • Eighth Edition • Introductory Chemistry Essentials • Sixth Edition • Modern Chemistry • Glencoe Science • Chemistry • Matter and Change

Chemistry

In this lesson, we will learn how to use the law of conservation of mass to calculate the masses of reactants and products in a chemical reaction.

Video

09:56

Sample Question Videos

01:28
04:01
03:46

Worksheet

Q1:

Yeast converts glucose to ethanol and carbon dioxide by anaerobic fermentation, as represented by the equation shown. In a particular fermentation process, 200.0 g of glucose is fully converted.

What is the total mass of ethanol and carbon dioxide at the end of the reaction?

If the fermentation process were carried out in an open container, would the mass of the container and contents increase, decrease, or stay the same?

If the reaction produces 97.7 g of carbon dioxide, what mass of ethanol is produced?

Q2:

Antoine Lavoisier was one of the first scientists to state the law of conservation of mass. When he heated a sample of tin and air in an airtight flask, tin reacted with oxygen in the air to produce tin oxide. Did the mass of the flask and its contents increase, decrease, or stay the same because of this reaction?

Q3:

Bread dough is placed in a baking tin and baked at . What happens to the mass of the bread?

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