AP Chemistry
3.4 Ideal Gas Law
A student injects a \(2.20\text{ g}\) sample of an unknown volatile liquid into a rigid, evacuated \(0.500\text{ L}\) container. The container is heated to \(300\text{ K}\), at which point all of the liquid completely vaporizes. The pressure of the gas inside the container is measured to be \(2.46\text{ atm}\). Assuming ideal gas behavior, what is the molar mass of the unknown substance?
Similar Questions
Tools for a 5
AP aligned mock tests to help you get a 5.
With grading, adaptive explanations, and more.
Find a Quiz
Find, solve, and grade every AP FRQ ever.
Find an FRQ
Stuck on AP Chemistry? Get unstuck with an AP specialist.1 to 1 tutors who know the exam inside out. Understand weeks of material in a single session.Book a SessionSee all our elite tutors
Learn AP Physics from scratch, quickly. This is the only course you'll need for the year.
A self-paced course with everything you need to get a 5. Trusted by over 15,000 students and 200+ schools. Learn fast, or we'll refund your purchase, backed by our 100% satisfaction guarantee.
Explore the Course