QuestionApril 30, 2025

Consider the following unbalanced reaction: KClO_(3)arrow KCl+O_(2) When 5.71 moles of KClO_(3) are consumed in the reaction above, how many grams of O_(2) are produced? Balance the equation first before plugging in to a formula. Round to 3 significant figures.

Consider the following unbalanced reaction: KClO_(3)arrow KCl+O_(2) When 5.71 moles of KClO_(3) are consumed in the reaction above, how many grams of O_(2) are produced? Balance the equation first before plugging in to a formula. Round to 3 significant figures.
Consider the following unbalanced reaction: KClO_(3)arrow KCl+O_(2) When 5.71 moles of KClO_(3) are consumed in the reaction above, how many grams of O_(2) are produced? Balance the equation first before plugging in to a formula. Round to 3 significant figures.

Solution
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Answer

274 grams of O_{2} are produced. Explanation 1. Balance the Chemical Equation The balanced equation is 2KClO_{3} \rightarrow 2KCl + 3O_{2}. 2. Calculate Moles of O_{2} Produced From the balanced equation, 2 moles of KClO_{3} produce 3 moles of O_{2}. Therefore, 5.71 moles of KClO_{3} will produce \frac{3}{2} \times 5.71 = 8.565 moles of O_{2}. 3. Convert Moles of O_{2} to Grams Use the formula **mass = moles × molar mass**. The molar mass of O_{2} is 32.00 g/mol. Thus, the mass of O_{2} is 8.565 \times 32.00 = 274.08 grams.

Explanation

1. Balance the Chemical Equation<br /> The balanced equation is $2KClO_{3} \rightarrow 2KCl + 3O_{2}$.<br /><br />2. Calculate Moles of $O_{2}$ Produced<br /> From the balanced equation, 2 moles of $KClO_{3}$ produce 3 moles of $O_{2}$. Therefore, 5.71 moles of $KClO_{3}$ will produce $\frac{3}{2} \times 5.71 = 8.565$ moles of $O_{2}$.<br /><br />3. Convert Moles of $O_{2}$ to Grams<br /> Use the formula **mass = moles × molar mass**. The molar mass of $O_{2}$ is 32.00 g/mol. Thus, the mass of $O_{2}$ is $8.565 \times 32.00 = 274.08$ grams.
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