I want to know whic n2 and co2 rms become same?
To determine at which temperature nitrogen dioxide (N2O) and carbon dioxide (CO2) have the same root mean square (rms) velocities, we need to calculate their respective velocities using the root mean square formula:
RMS velocity = √(3kT/m)
Where:
- k is the Boltzmann constant (1.38 x 10^-23 J/K)
- T is the temperature in Kelvin
- m is the molar mass in kilograms
First, let's find the molar masses of N2O and CO2:
- Molar mass of N2O (Nitrogen Dioxide) = 2(N) + 1(O) = 2(14.01 g/mol) + 1(16.00 g/mol) = 44.01 g/mol
- Molar mass of CO2 (Carbon Dioxide) = 1(C) + 2(O) = 1(12.01 g/mol) + 2(16.00 g/mol) = 44.01 g/mol
Since both N2O and CO2 have the same molar mass, they will have the same rms velocities at any given temperature.
If you specify a temperature, I can calculate the rms velocity for both N2O and CO2 at that temperature.