Balancing Combustion Reactions with Fractions

The video tutorial explains how to balance the chemical equation C4H6 + O2. It begins by counting the atoms on both sides of the equation, then balances the carbon and hydrogen atoms. The tutorial addresses the challenge of balancing oxygen atoms by using fractions and demonstrates how to convert these fractions into whole numbers for a balanced equation. The process is explained step-by-step, ensuring clarity in understanding the balancing of chemical equations.

What is the initial step in balancing the equation C4H6 + O2?

• Use fractions to balance the equation.

• Multiply the entire equation by 2.

• Count the atoms on both sides of the equation.

• Adjust the coefficient of H2O.

How many carbon atoms are present on the reactant side initially?

• Eight

• Six

• Four

• Two

What coefficient is placed in front of CO2 to balance carbon atoms?

• 5

• 4

• 3

• 2

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

• Seven

• Eight

• Nine

• Ten

What coefficient is used in front of H2O to balance hydrogen atoms?

• 2

• 3

• 5

• 4

What is the total number of oxygen atoms on the product side after balancing hydrogen?

• Nine

• Ten

• Twelve

• Eleven

What fraction is used to balance the oxygen atoms?

• 11/2

• 10/2

• 12/2

• 9/2

What is the purpose of multiplying the entire equation by 2?

• To increase the number of reactants.

• To balance hydrogen atoms.

• To balance carbon atoms.

• To eliminate fractions and use whole numbers.

What is the final coefficient in front of O2 after multiplying by 2?

• 12

• 9

• 10

• 11

Why is using fractions helpful in balancing combustion reactions?

• It makes the equation more complex.

• It increases the number of reactants.

• It decreases the number of products.

• It simplifies the process.