Final answer:
Yes, the question is based on Stoichiometry. In order to determine how many grams of KClO3 must be decomposed to produce 3.36 L of oxygen at STP, we need to use stoichiometry to relate the amount of oxygen gas to the amount of KClO3.
Step-by-step explanation:
Yes, the question is based on Stoichiometry. In order to determine how many grams of KClO3 must be decomposed to produce 3.36 L of oxygen at STP, we need to use stoichiometry to relate the amount of oxygen gas to the amount of KClO3. Here is the balanced chemical reaction for the decomposition of KClO3:
2KClO3 → 2KCl + 3O2
Using the balanced equation, we can set up a stoichiometry calculation to determine the amount of KClO3 needed:
mol KClO3 → mol O2 → L O2
Remember to use the ideal gas law to convert the volume of oxygen gas to moles if necessary.