To calculate the diffusion coefficient of oxygen in air at a given temperature and pressure, we can use the Chapman-Enskog equation, which is derived from the kinetic theory of gases. The equation is as follows:D = 3/16 * k * T / * ^0.5 * 1 / P where:D = diffusion coefficient m/s k = Boltzmann constant 1.38064852 10 J/K T = temperature K = pi 3.14159265359 = reduced mass of the gas pair kg P = pressure Pa First, we need to find the reduced mass of the gas pair, which is given by: = m1 * m2 / m1 + m2 where m1 and m2 are the molar masses of the two gases. In this case, we are considering the diffusion of oxygen O in air, which is primarily composed of nitrogen N . The molar masses of O and N are 32 g/mol and 28 g/mol, respectively. We need to convert these values to kg/mol:m1 = 32 g/mol * 1 kg / 1000 g = 0.032 kg/molm2 = 28 g/mol * 1 kg / 1000 g = 0.028 kg/molNow, we can calculate the reduced mass: = 0.032 kg/mol * 0.028 kg/mol / 0.032 kg/mol + 0.028 kg/mol = 0.000448 kg/molNext, we need to convert the pressure from atm to Pa:1 atm = 101325 PaNow, we can plug all the values into the Chapman-Enskog equation:D = 3/16 * 1.38064852 10 J/K * 298 K / 3.14159265359 * 0.000448 kg ^0.5 * 1 / 101325 Pa D 2.12 10 m/sTherefore, the diffusion coefficient of oxygen in air at a temperature of 298 K and a pressure of 1 atm is approximately 2.12 10 m/s.