# 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 This solution is **FREE** courtesy of BrainMass!

hi,

You use the ideal gas law equation correctly.

But you have to take care on the units.

In part A.) mmHg is used

In Part B.) and C.) atm. are used

You must transform it first from atm. to mmHg

1 atm. is equal to 760 mmHg.

So, we get:

2.0 atm. = 1400 mmHg

0.5 atm. = 380 mmHg

If you use these values in mmHg for p then you get the correct results.

Thanks for using BrainMass.com. Have a great day.

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