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

3 1/4 %

explanation:

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.