Balancing Chemical Equations Concepts

The video tutorial explains how to balance the chemical equation for the decomposition of zinc hydroxide into zinc oxide and water. It begins by counting the atoms on both sides of the equation, highlighting the importance of subscripts and parentheses in chemical formulas. The tutorial points out common mistakes, such as forgetting to account for all oxygen atoms, and emphasizes that the equation is already balanced. Dr. B concludes with a reminder of the balanced equation and thanks viewers for watching.

What are the products when zinc hydroxide decomposes?

• Zinc oxide and hydrogen

• Zinc oxide and water

• Zinc and oxygen

• Zinc and water

How many oxygen atoms are there in the reactant side of the equation?

• Four

• One

• Three

• Two

What does the subscript '2' in the formula Zn(OH)2 indicate?

• Two oxygen atoms only

• Two hydroxide ions

• Two zinc atoms

• Two hydrogen atoms only

Why is it important to consider the subscript when balancing equations?

• It affects the count of each type of atom

• It determines the state of matter

• It affects the number of molecules

• It changes the chemical properties

What is a common mistake when balancing the given equation?

• Overcounting hydrogen atoms

• Forgetting the zinc atom

• Ignoring the subscript

• Forgetting an oxygen atom on the product side

What is the final balanced equation for the decomposition of zinc hydroxide?

• Zn(OH)2 → ZnO + H2O

• Zn(OH)2 → Zn + O2 + H2

• Zn(OH)2 → ZnO2 + H2

• Zn(OH)2 → ZnO + H2