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Answer :
Final answer:
The mass of potassium chlorate needed to produce 35g of potassium chloride is found by setting up and solving a proportion based on the balanced chemical equation and molar masses of the compounds. However, the calculation gives a value of 57.9g which is not included in the provided answer options.
Explanation:
To solve this question, the balanced chemical equation for the decomposition of potassium chlorate (KClO3) into potassium chloride (KCl) and oxygen (O2) needs to be known. This is: 2KClO3 → 2KCl + 3O2. This tells us that 2 moles of potassium chlorate decompose to produce 2 moles of potassium chloride.
The molar masses of these compounds are calculated using atomic weights. The molar mass of KClO3 is 122.55 g/mol and the molar mass of KCl is 74.55 g/mol. Hence, 122.55 g of potassium chlorate will produce 74.55 g of potassium chloride.
To find out how many grams of potassium chlorate is needed to get 35g of potassium chloride, a proportion can be used:: 122.55 g of KClO3 / 74.55 g of KCl = x g of KClO3 / 35 g of KCl. Solving this equation for x gives x = 57.9 g which is not among the available answer options. Please double check the figures in the question.
Learn more about Chemical Stoichiometry here:
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