how many molecules of O2 may be produced from 50g of KClO3?
the formula is 2KClO3->2KCl+3O3
I just did this. What did you not understand? The grams of O in KClO3 is how many grams of O2 you get.
What does exactly conservation of mass mean?
To determine the number of molecules of O2 produced from 50g of KClO3, we need to use the given formula and the concept of stoichiometry.
First, we need to calculate the moles of KClO3 in 50g using its molar mass. The molar masses for each element are:
- K (potassium) = 39.1 g/mol
- Cl (chlorine) = 35.5 g/mol
- O (oxygen) = 16.0 g/mol
The molar mass of KClO3 is the sum of the molar masses of its constituent elements:
Molar mass of KClO3 = (2 * molar mass of K) + (1 * molar mass of Cl) + (3 * molar mass of O)
= (2 * 39.1) + 35.5 + (3 * 16.0)
= 39.1 + 35.5 + 48.0
= 122.6 g/mol
Next, we can calculate the moles of KClO3 in 50g using the formula:
moles = mass / molar mass
= 50g / 122.6 g/mol
≈ 0.408 mol
According to the balanced equation, 2 moles of KClO3 produce 3 moles of O2. Therefore, we can use the molar ratio to find the moles of O2 produced:
moles of O2 = (moles of KClO3) * (3 moles of O2 / 2 moles of KClO3)
= 0.408 mol * (3 / 2)
≈ 0.612 mol
Finally, we need to convert the moles of O2 to the number of molecules. One mole contains 6.022 × 10^23 molecules (Avogadro's number):
number of molecules = (moles of O2) * (6.022 × 10^23 molecules / 1 mole)
= 0.612 mol * (6.022 × 10^23 molecules / 1 mole)
≈ 3.69 × 10^23 molecules
Therefore, approximately 3.69 × 10^23 molecules of O2 can be produced from 50g of KClO3.