If a sample of a gas occupies 6.8 L at 327°C, what will be its volume at 27°C if the pressure does not change?

Answer 1

You would have to use the ideal gas law. We could have you memorize a bunch of equations that are derivites of this one but I rather you focus on this one and be able to derive the rest from here

PV=nrT

They gave you:

V₁: 6.8 L

T₁: 327 C°

V₂: Unknown

T₂: 27 C°

They said what happens to the volume if u change the temperature and keep the pressure the same.

We use P₁V₁/T₁=P₂V₂/T₂

_{since Pressure is the same we drop it from both sides!}

_{Leaving us:}

V₁/T₁=V₂/T_2. and solve the proportion

6.8/327=V₂/27

6.8(27)= 327(V₂)

Then divide both sides by 327 to isolate V₂

V₂= 0.56 L.

Always remember to keep ur units as you work through problem.

So if you decrease temperature you lower volume.

Answer 2

This is similar to another problem that I answered. Please reference that answer as this is another example of Charles' Law.

Use the equation V₁/T₁ = V₂/T₂

Covert the temperatures to Kelvin, substitute in the values into the equation, and solve for V₂. Let me know if you have any other questions.