Final answer:
None of the provided answer options for the amount of potassium chloride produced from the decomposition of 25.0 g potassium chlorate match the calculated theoretical yield of approximately 15.21 g. There may be a mistake in the question or the answer choices.
Step-by-step explanation:
Calculating the Theoretical Yield of Potassium Chloride
To find how many grams of potassium chloride are produced from the decomposition of 25.0 g of potassium chlorate, we need to use stoichiometry based on the balanced chemical equation for the decomposition of potassium chlorate (KClO3).
Firstly, we identify the relevant chemical equation: 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g). For every 2 moles of KClO3 that decompose, 2 moles of KCl are produced.
The molar masses of KClO3 and KCl are approximately 122.55 g/mol and 74.55 g/mol, respectively. This allows us to set up a proportion:
(25.0 g KClO3) / (122.55 g/mol) = (x g KCl) / (74.55 g/mol)
Therefore, x = (25.0 g KClO3 × 74.55 g/mol) / 122.55 g/mol
Solving for x gives us the theoretical yield of KCl, which is approximately 15.21 g. This means the maximum amount of KCl that can be obtained from 25.0 g of KClO3 is 15.21 g, assuming 100% yield.
However, none of the provided answer options (9.2 g, 5.4 g, 3.2 g, 2.8 g) match the calculated theoretical yield. There might be a mistake in the question or the answer options provided. Make sure to double-check the question and the answer options or consult additional resources.