2KClO3-2KCl+3O2
If this reaction produced 35.2 g of KCl, how much O2 was produced (in grams)?
Using the coefficients in the balanced equation lets you convert mols of mols of anything to anything in the equation.
mols KCl = grams/molar mass = approx 5 but that's an estimate.
5 mols KCl x (3 mols O2/2 mol KCl) = 5 x 3/2 = ? mols O2.
Then grams = mols o2 x molar mass O2.
To determine the amount of O2 produced in grams, we need to use stoichiometry, which involves the balanced chemical equation and the molar masses of the compounds involved.
Given the balanced chemical equation:
2KClO3 → 2KCl + 3O2
We can see that for every 2 moles of KClO3 reacted, we obtain 3 moles of O2. So, to calculate the amount of O2 produced, we need to convert the given mass of KCl to moles, and then use the stoichiometric ratios to find the moles of O2 produced. Finally, we convert the moles of O2 back to grams.
Step 1: Convert the mass of KCl to moles.
The molar mass of KCl is the sum of the atomic masses of potassium (K) and chlorine (Cl), which is:
K = 39.10 g/mol
Cl = 35.45 g/mol
Molar mass of KCl = 39.10 g/mol + 35.45 g/mol = 74.55 g/mol
To convert the mass of KCl to moles, we use the formula:
moles = mass / molar mass
moles of KCl = 35.2 g / 74.55 g/mol ≈ 0.471 moles
Step 2: Use the stoichiometric ratios to find the moles of O2 produced.
From the balanced equation, we know that:
2 moles KClO3 produce 3 moles O2
So, using the stoichiometric ratio:
moles of O2 = moles of KClO3 x (3 moles O2 / 2 moles KClO3)
moles of O2 = 0.471 moles x (3 moles O2 / 2 moles KClO3) ≈ 0.707 moles
Step 3: Convert moles of O2 to grams.
To convert moles of O2 to grams, we use the formula:
mass = moles x molar mass of O2
The molar mass of O2 is:
O = 16.00 g/mol (oxygen atomic mass)
molar mass of O2 = 2 x 16.00 g/mol = 32.00 g/mol
mass of O2 = 0.707 moles x 32.00 g/mol ≈ 22.6 grams
Therefore, approximately 22.6 grams of O2 were produced.