Nitrogen has relative molecular mass Mr = 28:0. Find the
root-mean-
square speed of nitrogen gas at 250 K.
Nitrogen has relative molecular mass Mr = 28:0. Find the root-mean- square speed of nitrogen gas...
At what temperature is the root-mean-square speed of nitrogen molecules equal to the root-mean-square speed of hydrogen molecules at 46 oC? (Hint: The molar mass of hydrogen atoms is 1.008 g/mol and of nitrogen atoms is 14.007 g/mol. The molar mass of H2 is twice the molar mass of hydrogen atoms, and similarly for N2.) The answer is in degree C.
(a) Compute the root-mean-square speed of a nitrogen molecule at 99.6°C. The molar mass of nitrogen molecules (N2) is 28.0x10-3 kg/mol. At what temperatures will the root-mean-square speed be (b) 1/3 times that value and (c) 2 times that value?
(a) Compute the root-mean-square speed of a nitrogen molecule at 74.7°C. The molar mass of nitrogen molecules (N2) is 28.0×10-3 kg/mol. At what temperatures will the root-mean-square speed be (b) 1/3 times that value and (c) 2 times that value?
The molecules of a certain gas sample at 375 K have a root-mean-square (rms) speed of 271 m/s. Calculate the most probable speed and the mass of a molecule. Most probable speed: Number 0 m/s Molecular mass: Number
Calculate the root-mean-square velocity of nitrogen gas at 273 K.
A certain gas sample has following speed distribution. The root mean square speed of this distribution is y=f(v) V(m/s) 250 450 380 m/s O a. 400 m/s Ob. 348 m/s 355 m/s O d.
Suppose that the root-mean-square velocity Us of water molecules (molecular mass is equal to 18.0 g/mol) in a flame is Feedback found to be 1170 m/s. What temperature does this represent? The root-mean-square velocity Urms of a molecule in a gas is related to 5.95 x109 temperature the mass of the molecule m and the temperature of the gas T. 3KT Urms The Boltzmann constant is k = 1.38 x 10-23 J/K.
3. For a sample of CO2 at 20 ºC, calculate the most probable molecular speed, mean molecular speed and root-mean-square molecular speed. Assume behavior described by the kinetic theory of gases. Also, what would the temperature need to increase to for each of the speeds in part (a) to double? [Hint: Look at the equations! No need for extensive calculations.]
4. Derive the expression for the root mean squared velocity of a gas from basic principles of mechanics. Explicitly list any assumptions that you make. Show that for an ideal gas PV = (1/3) n Mr v 2 ; n = number of moles, Mr = molecular mass and v = root mean square velocity
Calculate the root mean square speed for a sample of neon gas (Ne) at 298K. Your answer should have three significant figures. Use R=8.314 J/(K mol).