Oxygen has a molar mass of 32 g/mol. If 12 moles of oxygen are in a 0.1-m3 container with an rms speed of 480 m/s, what is the pressure of the gas?
I don't understand what I'm doing wrong Im using p=nM(vrms^2)/3V
and im getting 2.9E8?
someone pls explain
To calculate the pressure of a gas, you can use the ideal gas law equation, which states:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, you are given the number of moles (n = 12), the volume (V = 0.1 m^3), and the molar mass of oxygen (M = 32 g/mol). However, you need additional information to directly use the ideal gas law equation because the temperature (T) is not given.
The equation you mentioned, p = nM(vrms^2) / 3V, is the Maxwell-Boltzmann distribution equation used to determine the pressure of an ideal gas under certain conditions. Here, vrms represents the root mean square speed of the gas molecules.
To use this equation, you need to calculate vrms using the formula:
vrms = sqrt(3kT / M)
where k is the Boltzmann constant (k = 1.38 × 10^-23 J/K), T is the temperature in Kelvin, and M is the molar mass of the gas.
Since the temperature (T) is not given, you cannot directly calculate vrms and use it in the equation you mentioned. Therefore, the information provided is insufficient to calculate the pressure accurately.
Make sure to check if there is any missing information or any additional context needed to determine the temperature (T) in order to use the correct equation for calculating the pressure of the gas.