2KClO_(3)arrow 2KCl+3O_(2) If there are 45.82gKClO_(3) how many grams of O_(2) are made? (mmKClO_(3)=122g/mol)(mmO_(2)=32g/mol) 18.03 g KCI 59.028 KCI 27.21 g KCl 264920 g KCl

To solve this problem, we need to use the concept of stoichiometry and the molar mass of the substances involved.<br /><br />Given information:<br />- The balanced chemical equation is: $2KClO_{3} \rightarrow 2KCl + 3O_{2}$<br />- The mass of $KClO_{3}$ is $45.82g$<br />- The molar mass of $KClO_{3}$ is $122g/mol$<br />- The molar mass of $O_{2}$ is $32g/mol$<br /><br />Step 1: Calculate the number of moles of $KClO_{3}$.<br />Number of moles of $KClO_{3}$ = Mass of $KClO_{3}$ / Molar mass of $KClO_{3}$<br />Number of moles of $KClO_{3}$ = $45.82g / 122g/mol = 0.375 mol$<br /><br />Step 2: Use the stoichiometric relationship between $KClO_{3}$ and $O_{2}$ to find the number of moles of $O_{2}$ produced.<br />According to the balanced equation, 2 moles of $KClO_{3}$ produce 3 moles of $O_{2}$.<br />Number of moles of $O_{2}$ produced = $\frac{3}{2} \times 0.375 mol = 0.5625 mol$<br /><br />Step 3: Calculate the mass of $O_{2}$ produced.<br />Mass of $O_{2}$ = Number of moles of $O_{2}$ × Molar mass of $O_{2}$<br />Mass of $O_{2}$ = $0.5625 mol \times 32g/mol = 18.00g$<br /><br />Therefore, the correct answer is:<br />18.03 g $O_{2}$