Counting Atoms in Chemical Formulas With Coefficients and Subscripts

The video tutorial covers counting atoms in chemical formulas, focusing on acetic acid (CH3COOH) and methane (4 CH4). It explains how to use subscripts and coefficients to determine the number of atoms. The tutorial also discusses the law of conservation of mass, using the reaction of hydrogen and oxygen to form water (H2O) as an example. It highlights the importance of having equal numbers of atoms on both sides of a chemical equation to ensure it is balanced.

How many carbon atoms are present in the chemical formula for acetic acid (CH3COOH)?

• 3

• 2

• 4

• 1

In the formula CH3COOH, how many hydrogen atoms are there in total?

• 2

• 3

• 4

• 5

What is the total number of atoms in the chemical formula CH3COOH?

• 8

• 7

• 6

• 9

What does the coefficient in a chemical formula indicate?

• Number of molecules

• Number of atoms

• Number of compounds

• Number of elements

In the formula 4 CH4, how many hydrogen atoms are present in total?

• 8

• 12

• 20

• 16

What is the total number of atoms in the formula 4 CH4?

• 20

• 18

• 16

• 22

What does the law of conservation of mass state about chemical reactions?

• Mass is variable

• Mass is created

• Mass is destroyed

• Mass remains constant

In a balanced chemical equation, what should be equal on both sides?

• Number of molecules

• Number of compounds

• Number of atoms

• Number of elements

In the equation H2O yields H2 plus O2, how many oxygen atoms are on the product side?

• 3

• 1

• 2

• 4

Does the equation H2O yields H2 plus O2 follow the law of conservation of mass?

• Yes, it is balanced

• No, it is not balanced

• No, but with fewer atoms

• Yes, but with extra atoms