Balancing the Decomposition of Water Reaction

Dr. B explains how to balance the chemical equation for the decomposition of water into hydrogen and oxygen gas. Initially, the equation is unbalanced with unequal numbers of oxygen atoms. By adjusting the coefficients, Dr. B demonstrates how to balance both hydrogen and oxygen atoms, ensuring the equation is correct. The process involves placing a coefficient of 2 in front of H2O and H2 to achieve balance, resulting in equal numbers of hydrogen and oxygen atoms on both sides of the equation.

What is the initial imbalance observed in the decomposition of water reaction?

• Two hydrogen atoms and one oxygen atom on the product side

• Two hydrogen atoms and two oxygen atoms on the product side

• Two hydrogen atoms and one oxygen atom on the reactant side

• One hydrogen atom and two oxygen atoms on the reactant side

What is the first step taken to balance the oxygen atoms in the reaction?

• Adding a coefficient of 2 in front of H2O

• Adding a coefficient of 3 in front of H2O

• Removing an oxygen atom from the product side

• Adding a coefficient of 1 in front of H2O

After balancing the oxygen atoms, what is the next step to balance the equation?

• Add a coefficient of 3 in front of H2

• Add a coefficient of 1 in front of H2

• Add a coefficient of 2 in front of H2

• Add a coefficient of 4 in front of H2

How many hydrogen atoms are present on each side of the balanced equation?

• 4 hydrogen atoms

• 3 hydrogen atoms

• 2 hydrogen atoms

• 5 hydrogen atoms

How many oxygen atoms are present on each side of the balanced equation?

• 1 oxygen atom

• 2 oxygen atoms

• 4 oxygen atoms

• 3 oxygen atoms

What is the final balanced chemical equation for the decomposition of water?

• 2H2O -> H2 + 2O2

• 2H2O -> 2H2 + O2

• H2O -> H2 + O2

• H2O -> 2H2 + O2