To calculate the rate of diffusion of nitrogen gas in air, we can use Graham's law of diffusion, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. However, we need to find the molar mass of air first.Air is composed of approximately 78% nitrogen N2 , 21% oxygen O2 , and 1% argon Ar by volume. The molecular weights of N2, O2, and Ar are 28 g/mol, 32 g/mol, and 40 g/mol, respectively.To find the average molar mass of air, we can use the following equation:M_air = fraction of N2 M_N2 + fraction of O2 M_O2 + fraction of Ar M_Ar M_air = 0.78 28 g/mol + 0.21 32 g/mol + 0.01 40 g/mol M_air 28.97 g/molNow, we can use Graham's law of diffusion to find the rate of diffusion of nitrogen gas in air:Rate_N2 / Rate_air = M_air / M_N2 Rate_N2 / Rate_air = 28.97 g/mol / 28 g/mol Rate_N2 / Rate_air 1.018Since we are given the average velocity of nitrogen gas molecules 500 m/s , we can assume that this is the rate of diffusion of nitrogen in air:Rate_N2 = 500 m/sNow, we can find the rate of diffusion of air:Rate_air = Rate_N2 / 1.018Rate_air 491.16 m/sSo, the rate of diffusion of nitrogen gas in air at 25C and 1 atm pressure is approximately 500 m/s, while the rate of diffusion of air is approximately 491.16 m/s.