A gas is placed in a piston whose volume was $19.7 \cdot L$ $19.7L$ under a pressure of $0.95 \cdot a t m$ $0.95atm$ . If the volume were reduced to $22.5 \cdot L$ $22.5*L$ , what resultant pressure would develop?

Question

2906 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-12-19T02:03:09

The pressure of the system is 0.83 atm

To find the final pressure of the system we can use Boyle's Law:
![http://slideplayer.com/slide/5281881/]( useruploads.socratic.org )

Based on the information you've given me, we know the following variables:

$P_{1}$ $P_1$ = 0.95 atm
$V_{1}$ $V_1$ = 19.7 L
$V_{2}$ $V_2$ = 22.5 L
$P_{2}$ $P_2$ = $x$ $x$

Since we don't know what $P_{2}$ $P_2$ is, the equation has to be rearranged by dividing both sides by $V_{2}$ $V_2$ to get $P_{2}$ $P_2$ by itself:

$P_{2} = \frac{P_{1} \times V_{1}}{V_{2}}$ $P_2 = (P_1xxV_1)/V_2$

Now, just plug the given values into the equation:

$P_2 = (0.95 atm xx19.7cancelL)/(22.5cancelL)$

$P_2$ = 0.83 atm

A gas is placed in a piston whose volume was 19.7*L19.7⋅L19.7*L under a pressure of 0.95*atm0.95⋅atm0.95*atm. If the volume were reduced to 22.5*L22.5⋅L22.5*L, what resultant pressure would develop?