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Problem: An environmental engineer analyzes a sample of air contaminated with sulfur dioxide. To a 500.-mL sample at 700. torr and 38°C, she adds 20.00 mL of 0.01017 M aqueous iodine, which reacts as follows:SO2(g) + I2(aq) + H2O(l) ⟶ HSO4−(aq) + I−(aq) + H+(aq) [unbalanced]Excess I2 reacts with 11.37 mL of 0.0105 M sodium thiosulfate:I2(aq) + S2O32−(aq) ⟶ I−(aq) + S4O62−(aq) [unbalanced]What is the volume % of SO2 in the air sample?

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An environmental engineer analyzes a sample of air contaminated with sulfur dioxide. To a 500.-mL sample at 700. torr and 38°C, she adds 20.00 mL of 0.01017 M aqueous iodine, which reacts as follows:

SO2(g) + I2(aq) + H2O(l) ⟶ HSO4(aq) + I(aq) + H+(aq) [unbalanced]

Excess I2 reacts with 11.37 mL of 0.0105 M sodium thiosulfate:

I2(aq) + S2O32−(aq) ⟶ I(aq) + S4O62−(aq) [unbalanced]

What is the volume % of SO2 in the air sample?

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Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.