Question

A sample of an ideal gas has a volume of 3.60 L

at 12.80 ∘C
and 1.80 atm.
What is the volume of the gas at 20.20 ∘C
and 0.987 atm?

Answer 1

10.4

So first, remember the formula P1 × V1 ×T2 = P2 × V2 × T1.

P = Pressure

V = Volume

T = Temperature

(The Ones and Twos represent the measurements that came first and which came last, as you will see below)

Edit: Before solving, convert your temperatures to Kelvin first.

K = °C + 273

12.80°C = 285.8K

20.20°C = 293.2K

So, the first pressure and volume measurements with the second measurement of temperature are mutiplied.

(1.80 atm)(3.60 L)(293.2K)

That expression is equal to:

(0.987 atm)(V2)(285.8K)

So now we have:

(1.80 atm)(3.60 L)(293.2K)=(0.987 atm)(V2)(285.8K)

Mutiply everything on the left.

(1,899.936)=(0.987 atm)(V2)(285.8K)

Now, mutiply what you do have on the right.

(1,899.936)=(282.0846)(V2)

Then, from here, it's simple algebra.

Divide 1,899.936 ÷ 282.0846

You get 6.7353411

Dont forget to use Sig. figs.

so V2 = 6.74 L

That's your volume.