Boyle's Law considering different units for pressure
A sample of nitrogen has a volume of 50 L at a pressure of 760. mmHg. What is the volume of the gas at each of the following pressures if there is no temperature change.
A. 1500 mmHg (I have solves the problem for A!)
B. 2.0 atm.
C. .500 atm
According to my text book, the answers for P3 and P4, are 25 L and 100. L respectively. My answers to both questions are way off. I am using the correct formula of (P1*V1=P2*V2). I know that for this formula P1*V1/P2.
So my problem for B. should look like:
(50L)(760.mmHg)
________________
2.0 atm I need to know if I am right in setting up
this problem because I don't get tt the correct answers for B and C.
https://brainmass.com/chemistry/gas-laws/boyles-law-considering-different-units-pressure-36173
Solution Preview
hi,
You use the ideal gas law equation correctly.
But you have to take care on the units.
In part ...
Solution Summary
The solution desrcibes how different units for pressure must be transformed to get correct results when using Boyle's Law.
The current exercise uses the ideal gas equation and the way how to transform is given. The final calculation is not explicitly shown.