Posted by **Rosie829** on Monday, April 4, 2011 at 7:10pm.

With respect to Boyle's law (lab experiment with textbooks on an apparatus), if in the classroom the air pressure in the classroom is equal to 2.4 textbooks, how does one find the total pressure of a book with the volume of 26?

Am I on the right track by dividing the volume of a textbook by 2.4 (the air pressure in the classroom given by the Chemistry teacher)? Thank you for your valuable time!

## Answer this Question

## Related Questions

- English - What is in the classroom? 1. There is a blackboard in the classroom. 2...
- math - A textbook store sold a combined total of 462 biology and chemistry ...
- math - A textbook store sold a combined total of 315 physics and chemistry ...
- algebra - A textbook store sold a combined total of 205history and math ...
- Science (Chemistry) - The total pressure in a flask containing air and ethanol ...
- Chemistry - Would you expect the pressure of a 12.5 mL syringe of natural gas to...
- vapor pressure - The total pressure in a flask containing air and ethanol at 25....
- chemistry - The total pressure in a flask containing air and ethanol at 257C is ...
- chemistry - The total pressure in a flask containing air and ethanol at 257C is ...
- Chemistry - The total pressure in a flask containing air and ethanol at 257C is ...