To solve the problem, we need to find the molecular weight of gas Y given that the root mean square (rms) speed of gas X at 400 K is equal to the most probable speed of gas Y at 60 K. 1. Understand the formulas: - The formula for the root mean square speed (u_rms) of a...
To calculate the average, root mean square (RMS), and most probable velocities of nitrogen molecules at standard temperature and pressure (STP), we will use the following formulas:1. Average Velocity (Vavg): \( V{\text{av
The root mean square speed of one mole of a monoatomic gas having molecular mass M isUrms. The relation between the average kinetic energy (E ) of the gas andUrmsis : View Solution In the formulap=23E, the term (E) represents translational kinetic energy per unit volume of gas. ...
The formula for the most probable speed of a gas is given by: vmp=√2RTM 5. Calculate v_mp for Gas Y: Using the formula for gas Y: vmp=√2R⋅60M2=√120RM2 6. Set the Two Speeds Equal: According to the problem, the root mean square speed of gas X is equal to the most ...
Calculating the right-hand side: TN2=400⋅0.875=350K Step 8: ConvertTN2from Kelvin to Celsius. To convert Kelvin back to Celsius, we use: T(°C)=T(K)−273 Thus: TN2=350−273=77°C Final Answer: The temperature at which nitrogen molecules will have the same RMS velocity as ox...