Question

To calculate the mass of KClO_3 necessary to produce 1.23 g of O_2, we need to use the balanced chemical equation to relate the amount of O_2 produced to the amount of KClO_3 consumed. The balanced equation is:

2 KClO_3 -> 2 KCl + 3 O_2

Answer 1

To calculate the mass of KClO3 necessary to produce 1.23 g of O2, stoichiometry is used to relate the amounts through molar masses and the balanced chemical equation.

Step-by-step explanation:

To calculate the mass of KClO3 needed to produce 1.23 g of O2, we must use stoichiometry based on the balanced chemical equation. The balanced equation provided is: 2 KClO3 → 2 KCl + 3 O2. Using the molar masses (1 mol KClO3 = 122.55 g/mol and 1 mol O2 = 32.00 g/mol), we can relate the mass of KClO3 to the mass of O2 produced.

Step by Step Calculation

1. Calculate the moles of O2 produced using its molar mass (1.23 g / 32.00 g/mol).
2. Using the mole ratio from the balanced equation (2 moles of KClO3 for every 3 moles of O2), calculate the moles of KClO3 needed.
3. Convert the moles of KClO3 back to grams using its molar mass.

By following these steps, we can find the mass of KClO3 required to generate the given mass of oxygen gas.