Answer :
Final answer:
Using stoichiometric ratios from the balanced chemical equation 4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g) and the molar masses of KNO3 and O2, one can determine that to produce 56.4 kg of O2, approximately 84 kg of KNO3 must be decomposed. The correct answer is (B) 84 kg.
Explanation:
To answer your question about how many kilograms of potassium nitrate (KNO3) must be decomposed to produce 56.4 kg of O2 according to the reaction 4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g), we first need to understand the stoichiometry involved in this reaction.
From the balanced chemical equation, we can see that 4 moles of potassium nitrate (KNO3) yield 5 moles of O2 when they decompose.
Using this stoichiometric ratio, and the molar masses of KNO3 (101.1 g/mol) and O2 (32 g/mol), we can set up a proportion to find out the mass of KNO3 needed to produce your specified mass of O2.
4 moles of KNO3/5 moles of O2 = x kg of KNO3/56.4 kg of O2.
Here, x is the mass of KNO3 we are trying to find. Doing the math, we find that x equals approximately 84 kg.
So, according to the stoichiometry of the given chemical reaction, 84 kg of KNO3 must be decomposed to produce 56.4 kg of O2. The correct answer is (B) 84 kg.
Learn more about Stoichiometry here:
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