Balancing Chemical Reactions and Decomposition

The video tutorial explains how to balance the decomposition reaction of iron(II) sulfate, Fe2(SO4)3, into Fe2O3 and SO3. It begins by identifying the type of reaction and counting the atoms on both sides of the equation. The tutorial then demonstrates balancing the equation by adjusting the coefficients, focusing on sulfur and oxygen atoms, and ensuring the equation is balanced. Key points include understanding the application of subscripts and coefficients in chemical equations.

What type of reaction is the decomposition of iron(II) sulfate?

• Decomposition reaction

• Synthesis reaction

• Double replacement reaction

• Single replacement reaction

How many sulfur atoms are present in the reactant side of the equation?

• Four

• One

• Two

• Three

What is the total number of oxygen atoms on the reactant side before balancing?

• Six

• Nine

• Twelve

• Fifteen

Which element should be balanced first according to the video?

• Hydrogen

• Oxygen

• Sulfur

• Iron

What coefficient is placed in front of SO3 to balance sulfur atoms?

• One

• Four

• Two

• Three

After balancing, how many oxygen atoms are there on the product side?

• Fifteen

• Nine

• Six

• Twelve

What is the final balanced equation for the decomposition of iron(II) sulfate?

• Fe2(SO4)3 → Fe2O3 + 3SO3

• Fe2(SO4)3 → 2FeO + 3SO3

• Fe2(SO4)3 → FeO + SO3

• Fe2(SO4)3 → 2Fe2O3 + 3SO3

Why is it important to understand the application of coefficients in balancing equations?

• To change the chemical properties

• To ensure the equation is balanced

• To increase the reaction rate

• To decrease the reaction rate