What is the pressure (in atmospheres) of the gas inside the container connected to an open-end, mercury-filled manometer as shown in the picture? The atmospheric pressure is 0.95atm.

l----l |
(G) l |
l - ---
l Hg
l Hg *18cm
- - ---
Hg Hg
HgHgHgHg
what process do I use to solve for this problem? lost, tried and it didn't work out.

the picture didn't work. it is U shaped with Hg in the middle and an open end. The distance between the Hg, under the open air portion is 18cm, which is before the bottom of the U. Does that make sense. Basically a manometer.

To solve this problem, you can use the concept of hydrostatic pressure and the equation for the pressure exerted by a column of fluid. Here are the steps to follow:

1. Determine the difference in height of the mercury columns in the manometer.
- In this case, the height of the column on the left side is given as 18 cm.

2. Convert the height difference to the same unit as the pressure (atmospheres).
- Since 1 atm is equal to the pressure exerted by a column of mercury that is 76 cm high, you can use the following conversion factor:
1 atm = 76 cm Hg
So, divide the height difference (18 cm) by 76 cm Hg/atm to convert it to atmospheres.
18 cm / 76 cm Hg/atm = 0.2368 atm

3. Determine the pressure inside the container connected to the manometer.
- Since the left side of the manometer is open to the atmosphere, the pressure on that side is equal to the atmospheric pressure, which is given as 0.95 atm.

- The pressure inside the container can be determined by adding the pressure on the left side and the pressure difference between the two mercury columns:
Pressure inside container = Pressure on left side + Pressure difference

Pressure inside container = 0.95 atm + 0.2368 atm
Pressure inside container = 1.1868 atm

Therefore, the pressure of the gas inside the container is approximately 1.1868 atmospheres.