A5l container contains 3 moles of helium and 4 moles of hydrogen at a pressure of 9 atms maintaining a constant t and additional 2 mol or hydrogen are what is the new partial pressure of hydrogen gas in a container

7.71 atm

Explanation:

Given the following data:

According to the ideal gas law, we know that the product between pressure and volume of a gas is equal to the product between moles, the ideal gas law constant and the absolute temperature:

Since the temperature and the ideal gas constant are constants, as well as the fixed container volume of 5 L, we may rearrange the equation as:

This means for two conditions, we'd obtain:

Given:

Solve for the final pressure:

Now, according to the Dalton's law of partial pressures, the partial pressure is equal to the total pressure multiplied by the mole fraction of a component:

Knowing that:

And:

The equation becomes:

Substituting the variables:

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.