Amixture of nitrogen and hydrogen gases, at a total pressure of 663 mm hg, contains 3.46 grams of nitrogen and 0.156 grams of hydrogen. what is the partial pressure of each gas in the mixture? pn2 = mm hg ph2 = mm hg

The partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

Explanation:

To calculate the number of moles, we use the equation:

Given mass of nitrogen gas = 3.46 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in above equation, we get:

Given mass of hydrogen gas = 0.156 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in above equation, we get:

Mole fraction of a gas is calculated by using the formula:

     ......(1)

Putting values in equation 1, we get:

Putting values in equation 1, we get:

The partial pressure of a gas is given by Raoult's law, which is:

    ......(2)

where,

= partial pressure of substance A

= total pressure  = 663 mmHg

= mole fraction of substance A

Hence, the partial pressure of nitrogen gas is 405.76 mmHg and that of hydrogen gas is 257.24 mmHg

icc, international association for cereal chemistry