QuestionApril 30, 2025

Consider the following reaction: O_(2)+2SO_(2)arrow 2SO_(3) How many moles of O_(2) are consumed when 3.1 moles of SO_(3) are produced in the reaction above? Round to 3 significant figures.

Consider the following reaction: O_(2)+2SO_(2)arrow 2SO_(3) How many moles of O_(2) are consumed when 3.1 moles of SO_(3) are produced in the reaction above? Round to 3 significant figures.
Consider the following reaction: O_(2)+2SO_(2)arrow 2SO_(3) How many moles of O_(2) are consumed when 3.1 moles of SO_(3) are produced in the reaction above? Round to 3 significant figures.

Solution
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Answer

1.55 moles of O_2 are consumed. Explanation 1. Determine the mole ratio From the balanced equation, the mole ratio of O_2 to SO_3 is 1:2. 2. Calculate moles of O_2 consumed Use the mole ratio to find moles of O_2: \text{moles of } O_2 = \frac{1}{2} \times \text{moles of } SO_3 = \frac{1}{2} \times 3.1 = 1.55 moles.

Explanation

1. Determine the mole ratio<br /> From the balanced equation, the mole ratio of $O_2$ to $SO_3$ is 1:2.<br /><br />2. Calculate moles of $O_2$ consumed<br /> Use the mole ratio to find moles of $O_2$: $\text{moles of } O_2 = \frac{1}{2} \times \text{moles of } SO_3 = \frac{1}{2} \times 3.1 = 1.55$ moles.
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