Density of mixture of oxygen and nitrogen is 1.28 gm/lit at stp. Calculate partial pressure of oxygen.

According to dalton' for partial pressure formula is partial pres.= vapour pres.* mole fraction of component so we can't get partial pressure of component from density (jay hind)

To calculate the partial pressure of oxygen in the mixture, you need to know the mole fraction of oxygen in the mixture, as well as the total pressure of the system. The mole fraction can be calculated using the ideal gas law.

The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L atm/mol K), and T is the temperature in Kelvin.

At STP (Standard Temperature and Pressure), the temperature is 273.15 K, and the pressure is 1 atm. Given the density of the mixture (1.28 g/L), we can calculate the molar mass of the mixture.

The molar mass of the mixture can be calculated using the equation:

Molar mass = (density * molar mass of air) / (density of air)

The molar mass of air is approximately 28.97 g/mol, and the density of air at STP is approximately 1.225 g/L. Using these values, we can calculate the molar mass of the mixture:

Molar mass of mixture = (1.28 g/L * 28.97 g/mol) / 1.225 g/L

Next, we need to determine the mole fractions of oxygen and nitrogen in the mixture. Let's assume the mole fraction of oxygen is x, which means the mole fraction of nitrogen would be (1 - x).

From the equation:

Molar mass of mixture = x * Molar mass of oxygen + (1 - x) * Molar mass of nitrogen

We can rearrange the equation to solve for x:

(x * Molar mass of oxygen) + ((1 - x) * Molar mass of nitrogen) = Molar mass of mixture

Substituting the molar mass of oxygen (16 g/mol) and nitrogen (28 g/mol), we can solve for x.

Once we determine the mole fraction of oxygen (x), we can calculate the partial pressure of oxygen using Dalton's law of partial pressures:

Partial pressure of oxygen = Mole fraction of oxygen * Total pressure

Given that the total pressure is 1 atm, we can substitute the values and calculate the partial pressure of oxygen.