Question

A sample of helium gas has a volume of 250.0 mL when it pressure is 0.935 atm. If the

temperature remains constant, what will the pressure of the gas be when it has a volume of
175.0 mL?

Answer 1

The answer is

1.336 atm

Step-by-step explanation:

In order to find the volume of the gas at 175 mL we use the Boyle's law formula

That's

`P _1 V _1 = P _2 V _2`

where

P1 is the initial pressure

V1 is the initial volume

V2 is the final volume

P2 is the final pressure.

Since we are finding the final pressure

`P _2 = (P _1 V _1)/( V _2)`

From the question

P1 = 0.935 atm

V1 = 250.0 mL

V2 = 175 mL

Substitute the values into the above formula and solve

That's

`P _2 = (0.935 * 250)/(175) \\ = (233.75)/(175) \\ = 1.33571`

We have the final answer as

1.336 atm

Hope this helps you