CHEM 1A

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?

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asked by Chad
  1. 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.

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    posted by DrBob222
  2. Sweet, Thank you....

    1. 0
    posted by Chad

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