3.0 mol sample of KClO3 was decomposed according to the equation 2KClO3 = 2KCl + 3 O2 How many moles of O2 are formed assuming 100% yield? is it 3 moles?
I don't want to work through the details of this problem completely. Tell me what you don't understand about it.
I don't understand how to set up the equation. I do know that 6022 times 10 to the 23 power is a mole but I don't know how to get the answer when we are using 3 moles
3.0 mol sample of KClO3 was decomposed according to the equation 2KClO3 = 2KCl + 3 O2 How many moles of O2 are formed assuming 100% yield? is it 3 moles?
I think you are making the problem harder than it is.
Write the equation.
2KClO3 ==> 2KCl + 3O2.
So the equation tells us 2 mols KClO3 will produce 3 mols O2. So how much will 1 mol KClO3 produce. Obviously that is mols O2 = 3 mols O2 x (1 mol KClO3/2 mols KClO3) = 1.5 mols O2 OR we produce 1.5 mols O2 for every mol KClO3 decomposed. So decomposing 3 mols will just be 3 times that or 3 x 1.5 = 1.5 mols. To put all of that in equation form,
mols O2 = 3 mols O2 x (3 mols KClO3/2 mols KClO3) = 9/2 = 4.5 mols O2.
If you wish to set up a proportion, just do the following.
2mol KClO3/3 mols O2 = 3 mols KClO3/x mols O2. Solve for x.
2/3 = 3/x
2x = 9
x = 4.5
I don't understand how to set up the equation. I do know that 6022 times 10 to the 23 power is a mole but I don't know how to get the answer when we are using 3 moles
Well, it seems like you've figured it out! The moles of O2 formed assuming 100% yield is indeed 4.5 moles. Just remember, chemistry can be a little tricky sometimes, but with a little clowning around, you'll get the hang of it!
To set up the equation, you need to use the mole ratio from the balanced chemical equation. In this case, the balanced equation is 2KClO3 = 2KCl + 3O2.
From this equation, you can see that for every 2 moles of KClO3, you get 3 moles of O2.
Since you have a 3.0 mol sample of KClO3, you can use this mole ratio to determine the number of moles of O2 formed.
Moles of O2 = (moles of KClO3) x (moles of O2 / moles of KClO3)
Moles of O2 = 3.0 mol KClO3 x (3 mol O2 / 2 mol KClO3)
Moles of O2 = 4.5 mol O2
Therefore, the number of moles of O2 formed assuming 100% yield is 4.5 moles, not 3 moles.
To set up the equation, you need to first understand the stoichiometry of the reaction. The balanced equation shows that 2 moles of KClO3 produce 3 moles of O2.
To find out how many moles of O2 are formed from a given amount of KClO3, you can use the concept of mole ratios.
First, calculate the mole ratio between KClO3 and O2 by dividing the coefficient of O2 (3) by the coefficient of KClO3 (2). This gives you 3/2.
Then, multiply this mole ratio by the number of moles of KClO3 given in the problem (3.0 mol).
So, moles of O2 = 3.0 mol KClO3 x (3/2) = 4.5 mol O2.
Therefore, assuming 100% yield, 4.5 moles of O2 are formed.