If $9 L$ of a gas at room temperature exerts a pressure of $12 kPa$ on its container, what pressure will the gas exert if the container's volume changes to $4 L$ ?

Question

2641 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-07-24T03:21:45

$color(purple)("27 kpa"$

Let's identify our knowns and unknowns:

The first volume we have is $9 L$ , the first pressure is $12kPa$ , and the second volume is $4L$ . Our only unknown is the second pressure.

We can ascertain the answer using Boyle's Law:
![slideplayer.com]( useruploads.socratic.org )

Rearrange the equation to solve for $P_2$

We do this by dividing both sides by $V_2$ in order to get $P_2$ by itself:
$P_2=(P_1xxV_1)/V_2$

Now all we have to do is plug in the given values:
$P_2=(12\kPa xx 9\ cancel"L")/(4\cancel"L")$ = $27 kPa$

If 9 L9 L of a gas at room temperature exerts a pressure of 12 kPa12 kPa on its container, what pressure will the gas exert if the container's volume changes to 4 L4 L?