Question

A mixture of hydrogen (2.02 g) and chlorine (35.90 g) in a container at 300 K has a total gas pressure of 748 mm Hg. What is the partial atmospheric pressure (atm) of hydrogen in the mixture?

Answer 1

The partial atmospheric pressure (atm) of hydrogen in the mixture is 0.59 atm.

How do we calculate the partial pressure of gas?

Partial pressure of particular gas will be calculated as:

p = nP, where

• P = total pressure = 748 mmHg
• n is the mole fraction which can be calculated as:
• n = moles of gas / total moles of gas

Moles will be calculated as:

• n = W/M, where
• W = given mass
• M = molar mass

Moles of Hydrogen gas = 2.02g / 2.014g/mol = 1 mole

Moles of Chlorine gas = 35.90g / 70.9g/mol = 0.5 mole

Mole fraction of hydrogen = 1 / (1+0.5) = 0.6

Partial pressure of hydrogen = (0.6)(748) = 448.8 mmHg = 0.59 atm

Hence, required partial atmospheric pressure of hydrogen is 0.59 atm.

To know more about partial pressure, visit the below link:
brainly.com/question/15302032

#SPJ1