Question

In an experiment, 125ml of H2 is collected over water at 27C and barometric pressure of 753 torr. the vapor pressure of water at 27C is 26.74 what is the partial pressure of H2?

Answer 1

To calculate the partial pressure of hydrogen gas collected over water, subtract the vapor pressure of water (26.74 torr) from the total pressure (753 torr), resulting in a partial pressure of 726.26 torr for H2.

Step-by-step explanation:

The student's question is related to the calculation of the partial pressure of hydrogen gas (H2) when collected over water. The experiment provided the conditions of a total pressure at 753 torr and a temperature of 27°C, with the water's vapor pressure being 26.74 torr at this temperature. To find the partial pressure of the hydrogen gas, we subtract the vapor pressure of water from the total barometric pressure:

Partial pressure of H2 = Total pressure - Vapor pressure of water

Partial pressure of H2 = 753 torr - 26.74 torr = 726.26 torr

Therefore, the partial pressure of the hydrogen gas collected over water is 726.26 torr.

Answer 2

Partial pressure of H₂ = 0.9556 atm

Step-by-step explanation:

Given:

Barometric pressure = 753 torr

Vapor pressure of water = 26.74 torr

FInd:

Partial pressure of H₂

Computation:

Partial pressure of H₂ = Barometric pressure - Vapor pressure of water

Partial pressure of H₂ = 733 - 26.74

Partial pressure of H₂ = 726.26 torr

1 atm = 760 torr

So,

Partial pressure of H₂ = 726.26/760

Partial pressure of H₂ = 0.9556 atm