Using the following equation, how many moles of KClO3 are required to form 6.9 moles of O2?

Answer: To determine how many moles of KClO_3 are required to produce 6.9 moles of O_2, you would first need to know the balanced chemical equation for the decomposition of potassium chlorate (KClO_3). The balanced equation is as follows:

2 KClO_3 → 2 KCl + 3 O_2

This equation tells us that from 2 moles of KClO_3, we can get 3 moles of O_2.

Now, you want to find out how many moles of KClO_3 would be needed to produce 6.9 moles of O_2. To do this, you can set up a ratio using the stoichiometry from the balanced equation:

(2 moles KClO_3) / (3 moles O_2) = (x moles KClO_3) / (6.9 moles O_2)

Now, solve for x:

x = (6.9 moles O_2) * (2 moles KClO_3) / (3 moles O_2) x = 13.8 / 3 x = 4.6 moles KClO_3

Therefore, you would need 4.6 moles of KClO_3 to produce 6.9 moles of O_2.

Extra: Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data. In stoichiometry, the coefficients in a balanced chemical equation are used to form mole-to-mole conversion factors, which allow you to calculate the amount of products that will form or the amount of reactants needed for a reaction to occur.

For the decomposition of potassium chlorate into potassium chloride and oxygen, the balanced chemical equation provides key information. The coefficients (2 for KClO_3 and 3 for O_2) indicate that 2 moles of potassium chlorate produce 3 moles of oxygen gas, which is a mole ratio of 2:3. This mole ratio is essential for stoichiometric calculations, allowing you to convert between moles of different substances in a chemical reaction.