Question

Mercury is used in a barometer due to its high density. Suppose another liquid with half the density of mercury was used in a barometer. What would be the normal atmospheric pressure with this barometer? Give a brief explanation for your answer.

Answer 1

506464 g/(cm*s^2)

Step-by-step explanation:

Atmospheric pressure is defined as the pressure caused by the mass of the gaseous atmosphere. With the use of mercury, atmospheric pressure = mercury density × acceleration due to gravity × height of column of mercury.

Normally, density of mercury = 13.6 ×density of water

If the density of water =
`1 g/cm^(3)`

Thus, density of mercury =
`13.6 g/cm^(3)`

column of mercury = 760 mm = 76 cm

Acceleration due to gravity = 9.8
`m/s^(2) = 980 cm/s^(2)`

Therefore:

Atmospheric pressure = 13.6*76*980 = 1012928 g/(cm*s^2)

If a liquid with half the density of mercury is used, the atmospheric pressure will be equal to 1012928/2 = 506464 g/(cm*s^2)