Answered: Find the K.E. (1) per cm³ (2) per mole… | bartleby

Related questions

Question

Find the K.E. (1) per cm³ (2) per mole
(3) per gram and (4) per molecule of nitrogen at
N.T.P. (Molecular weight of N₂ 28, Normal
pressure = 76 cm of mercury, density of Hg
13.6 gm/cm³ g = 980 cm/s², Avogadro's number
6.023 x 1023 molecules/mole. (R = 8.314 x 10²
erg/mole K)

Expert Solution

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Blurred answer

Similar questions

The concentration of a frictionless fluid flowing through a channel is measured with a diffusion constant, D = 4.5E-3 m2/s at room temperature. The radius and length of the channel are given as r = 9.2E-2 m and 2.2 m, respectively. Hint: (KB = 1.3806E-23 m2.kg.s-2.K-1, T = 273 K).(a) Calculate the gradient of concentration of the fluid given the initial and final concentrations as C1 = 70 kg/m3 and C2 = 22 kg/m3, respectively.(b) Estimate the coefficient of viscosity of blood
The volume of an automobile tire is 2.5 × 10−2m3 . the pressure of the air in the tire is 3 atm and the temperature is 37C ◦ . what is is the mass of air in grams ? The mean molecular mass of air is 29g. 1 atm = 1.01 × 105 Pa ; Calculate to 2 decimals.
If the velocities of three molecules are 2 m/s, 3 m/s, 4 m/s respectively. Then the root mean square velocity is, (a) 4 m/s (b) . 3.01 m/s (с) 3m/s (d) 5 m/s
a) Calculate the volume in ft of one Ib-mole of air (MW = 29 lbm/lb-mole) at a temperature of 492 R at a pressure of 1 atm (absolute). b) Repeat the calculation of a) but now considering 1 Ib-mole of CO2 (MW= 44 lbmlb-mole). c) Calculate the molar volume (V) of this mole of air in ft'/lb-mole. d) Calculate the density (P) of air in Ibm/ft under these conditions e) Calculate the density (p) of CO, in Ib.m/ft under these conditions
1. The figure shows the natural loga- rithm of the particle density of air (p = 1.225 kg m-3 at h = 0) for a constant temperature. Given that the linear fit to the data is In(n) = 58.533 at h = 0 and In(n) 57.386 at h = 10ª m, stating any assumptions used, 10 2000 4000 6000 8000 Height, h [m] (a) calculate the average mass of an air particle, (b) determine the temperature of the air. Number density, In(n) [m] 57.5 58 58.5
The vapor pressures of the components, A and B, in a binary solution have been modeled and found to obey хара exp(0.75 XB) A A exp(0.75x) where XÃ and are the mole fractions, and PA* and PB* are the vapor pressures of each pure substance at room temperature. (a) If PA* = 0.084 bar and the total pressure of a mixture with XA = 0.40 is 0.125 bars, what is PB*, the vapor pressure of pure B (in bars)? P = X P А P₁ = X_P B QUESTION 14 B B * * Continuation of the previous problem (b) Assuming that the vapor is an ideal gas, what is the mole fraction of component B in the vapor phase?
Please help me
A bubble of air is rising from the sea floor, from a depth of about 500 m. At this depth the pressure is 5.1*106 Pa (about 50.3 atm) and is at a temperature of about 7.0° C. It rises to the surface with the atmosphere, at a temperature of 20° C. If the bubble is observed to have a volume of 4 cm³ at the surface, what was its volume at the sea floor? Assume the number of moles of gas in the bubble is constant. B.
Calculate: (a) the number of moles in 1.00 m3 of gas at STP, and (b) the number of liters of gas per mole.
A sample of argon gas is in a container at 35.0° C and 1.22 atm pressure. The radius of an argon atom (assumed spherical) is 0.710 x 10-10 m. calculate the available volume for each atom.
At what height is the atmospheric pressure 29.0% of what it is at sea level? Assume the molar mass of the air molecules to be 29.0 g/mol and that the air temperature is uniformly 287 K. [Answer in kilometres with 3 sig digits, but do not enter units with your answer]
I need the answer quickly

SEE MORE QUESTIONS