TWO IDENTICAL NANO METERS ARE FILLED WITH MERCURY. THE NANO METERS ARE PLACED IN A CLOSED PRESSURIZED BOX CONTAINING AIR AT 1,000 TORR PRESSURE. ONE NANO-METER CONTAINS GAS a, AND THE OTHER GAS B. WHAT IS THE DIFFERENCE BETWEEN THE PRESSURES OF THE TWO GASES? THE DENSITY IS 13.6 G/CM^3
a.) 10 TORR
B.)30 TORR
C.)60 TORR
D.) 90 TORR
E.) 120 TORR
Nano meters? Surely you don't mean that. Could it be manometer? (pronounced man nom eter)
now your question: Something is missing here. There has to be some level of Hg involved.
yes
i meant manometer
To find the difference between the pressures of gas A and gas B, we can use the concept of partial pressure and Dalton's law of partial pressures.
According to Dalton's law, the total pressure is equal to the sum of the partial pressures of the individual gases in a mixture. In this case, the total pressure is 1,000 Torr.
Let's consider the two scenarios separately:
Scenario 1: Nano-meter containing gas A
The pressure exerted by gas A is the partial pressure of A. Let's denote it as PA. Since the total pressure is 1,000 Torr, the pressure exerted by gas B would be the remaining pressure:
PB = Total pressure - PA = 1,000 Torr - PA
Scenario 2: Nano-meter containing gas B
Similarly, the pressure exerted by gas B is the partial pressure of B, denoted as PB. Again, the pressure exerted by gas A would be the remaining pressure:
PA = Total pressure - PB = 1,000 Torr - PB
The difference between the pressures of the two gases is the difference between PA and PB. Therefore, we can write:
PA - PB = 1,000 Torr - PB - PA
PA - PB = 1,000 Torr - 2PA
To proceed further, we need additional information such as the ratio of the volumes of the nano-meters or the molar ratios of the gases A and B. The densities of the gases and the density of mercury are not relevant to finding the pressure difference.
As it stands, we cannot determine the difference between the pressures of the two gases without additional information.