Question

Question #b100e

Answer 1

`"150. kPa"`

Explanation:

For starters, I will assume that the problem meant

...note that the gas had double the volume when she started...

Now, Jessica's in luck because she can use Boyle's Law to find the initial pressure of the gas.

The idea here is that the temperature and number of moles of gas are being kept constant in the experiment, which means that you can use the direct relationship that exists between pressure and volume described by Boyle's Law.

Simply put, when temperature and number of moles of gas are being kept constant, increasing the pressure of the gas will result in a decrease in volume.

Likewise, decreasing the pressure of the gas swill result in an increase in volume.

![http://www.peoi.org/Courses/Coursessp/chemintro/contents/frame6c.html]()

Now, Jessica knows that the gas had double the volume before the experiment started, which means that the volume of the gas got halved.

If you take `V_1` to be the initial volume of the gas, you can say that the final volume of the gas, `V_2`, will be

`V_2 = 1/2 * V_1" " " "color(orange)("(*)") ->` the volume of the gas got halved

Mathematically, Boyle's Law can be expressed like this

`color(blue)(|bar(ul(color(white)(a/a)P_1V_1 = P_2V_2color(white)(a/a)|)))" "`, where

`P_1`, `V_1` - the pressure and volume of the gas at an initial state
`P_2`, `V_2` - the pressure and volume of the gas at a final state

Your job here is to solve for `P_1`, the initial pressure of the gas. Rearrange the equation to isolate `P_1`

`P_1V_1 = P_2V_2 implies P_1 = V_2/V_1 * P_2`

Use equation `color(orange)("(*)")` and plug in the value you have for the final pressure of the gas to get

`P_1 = (1/2 * color(red)(cancel(color(black)(V_1))))/color(red)(cancel(color(black)(V_1))) * "300. kPa" = 1/2 * "300. kPa" = color(green)(|bar(ul(color(white)(a/a)"150. kPa"color(white)(a/a)|)))`

Now, does this result make sense?

According to Boyle's Law, a decrease in volume is the result of an increase in pressure. It thus follows that doubling the pressure of the gas would cause the volume to be halved.