Question

consider the flasks in the following diagram. what are the final partial pressures of h2 and n2 after the stopcock between the two flasks is opened? (assume the final volume is 3.00 l.) what is the total pressure (in torr)?

Answer 1

The final partial pressures of
`H_2` and
`N_2` are 316.67 torr and 50.67 torr, respectively, and the total pressure is 367.33 torr.

The final partial pressures of
`H_2` and
`N_2` after the stopcock between the two flasks is opened can be calculated using the ideal gas law, which states that the pressure of a gas is directly proportional to its volume.

Given that the initial volume of
`H_2` is 2.00 L and its initial pressure is 475 torr, when the volume increases to 3.00 L, the final pressure of
`H_2` (
`PH_2`) can be calculated as follows:

`PH_2` = (Initial Pressure of
`H_2` * Initial Volume of
`H_2`) / Final Volume

`PH_2` = (475 torr * 2.00 L) / 3.00 L

`PH_2` ≈ 316.67 torr

Similarly, the initial volume of
`N_2` is 1.00 L and its initial pressure is 0.200 atm. Converting this pressure to torr (since 1 atm = 760 torr), we get an initial pressure of 152 torr for
`N_2`. When the volume increases to 3.00 L, the final pressure of
`N_2` (P
`N_2`) can be calculated as follows:

P
`N_2` = (Initial Pressure of
`N_2` * Initial Volume of
`N_2`) / Final Volume P
`N_2`

= (152 torr * 1.00 L) / 3.00 L

P
`N_2` ≈ 50.67 torr

The total pressure in the system after the stopcock is opened is the sum of the partial pressures of
`H_2` and
`N_2`:

Total Pressure =
`PH_2` +
`PN_2`

Total Pressure = 316.67 torr + 50.67 torr

Total Pressure ≈ 367.33 torr

So, the final partial pressures of
`H_2` and
`N_2` are approximately 316.67 torr and 50.67 torr, respectively, and the total pressure is approximately 367.33 torr