Problem: In preparation for a demonstration, your professor brings a 1.5-L bottle of sulfur dioxide into the lecture hall before class to allow the gas to reach room temperature. If the pressure gauge reads 85 psi and the temperature in the classroom is 23°C, how many moles of sulfur dioxide are in the bottle? (Hint: The gauge reads zero when the gas pressure in the bottle is 14.7 psi.)

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Use the ideal gas equation to solve for the number of moles of sulfur dioxide in the bottle.

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Problem Details

In preparation for a demonstration, your professor brings a 1.5-L bottle of sulfur dioxide into the lecture hall before class to allow the gas to reach room temperature. If the pressure gauge reads 85 psi and the temperature in the classroom is 23°C, how many moles of sulfur dioxide are in the bottle? (Hint: The gauge reads zero when the gas pressure in the bottle is 14.7 psi.)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hatfield's class at UIC.

What textbook is this problem found in?

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.