Question

What mass in grams are produced when a ? are completely reacted according to the following chemical equation: 2 KClO₃ (s) → 2KCl (s) + 3o₂ (g)?

Answer 1

The mass of oxygen gas produced from the decomposition of potassium chlorate can be found through stoichiometric calculations, but the starting mass of the reactant KClO₃ must be known to provide a specific answer.

Step-by-step explanation:

To determine the mass of oxygen gas (O₂) produced when potassium chlorate (KClO₃) is decomposed, we can follow the steps of stoichiometric calculations. Given the balanced chemical equation 2 KClO₃ (s) → 2 KCl (s) + 3 O₂ (g), it shows that 2 moles of KClO₃ produce 3 moles of O₂. Using the provided molar masses, we have:

• 1 mol KClO₃ = 122.55 g/mol
• 1 mol O₂ = 32.00 g/mol

First, you would convert the mass of KClO₃ to moles, then use the stoichiometry of the reaction to find out how many moles of O₂ are produced. Afterward, convert the moles of O₂ to grams using its molar mass, which is the theoretical yield of O₂ in grams.

Here is an example to demonstrate the process:

1. Convert the given mass of KClO₃ to moles using its molar mass.
2. Use the mole ratio from the balanced equation to determine moles of O₂ produced.
3. Convert moles of O₂ to mass (g) using the molar mass of O₂.

Unfortunately, the exact starting mass of KClO₃ is not provided. We require this to solve for the mass of O₂ produced.