Asked by Chad

Balanced equation,
4KNO3(s) ----->2K2O(s) + 2N2(g) + 5O2(g)
To produce 51.8kg of O2,
How many moles of KNO3 must be heated?

How many grams of KNO3 must be heated?

Do you calculate like KNO3 and O2 is just one mole or do you divide 4/5 at the end of the equation?

51.8kgO2 x 1000g/1kg = 51800g O2 / 32.00g O2 = 1618.75g x 4/5 = 1295 moles KNO3...Is this correct?
Answered by DrBob222
On the right track but not quite right. You may have just mislabeled your numbers.
51,800 g O2 is what you want.
mols O2 = 51,800/32 = 1618.7 MOLES O2 (not grams) needed. Convert that to mols KNO3 by multiplying by 4/5 = 1295 mols KNO3 and you have that labeled right.

Then grams KNO3 = mols KNO3 x molar mass KNO3.
Answered by Chad
Sweet, Thank you....
Answered by carly
What type of chemical reaction is this?



4KNO3 -> 2K2O + 2N2 + 5O2
Answered by savanna
What type of chemical reaction is this?



4KNO3 -> 2K2O + 2N2 + 5O2
There are no AI answers yet. The ability to request AI answers is coming soon!