The Z factor is approximately the same for all gases at the same reduced temperature and reduced pressure.
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The Z factor is approximately the same for all gases at the same reduced temperature and reduced pressure.
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- By what factor does the rms speed of a molecule change if the temperature is increased from 24 °C to 1000 °C? VD ΑΣΦ Submit Request Answer ?Consider a gas that follows the equation of state NRT aN² 2 P V - bN V2 This is called van der Waals gas (a,b > 0). For temperatures T > Tc : monotonically decreasing function. Assume T > Tc and Cy = 3NR/2. = 8a p(V) is a 27Rb Consider an insulated box with volume V₁. The box was divided by a wall. One of the compartments had volume Vo at temperature To, which was filled with van der Waals gas of amount N. The other compartment was vacuum. The system was in equilibrium. (i) The wall was removed abruptly. The gas expanded and occupied the entire box. This process is called adiabatic free expansion. The temperature in the box is now T₁ in equilibrium. What is T₁ - To? (ii) The internal energy of the gas does not change by adiabatic free expansion. Why? (iii) Instead of the abrupt removal, the wall was moved through adiabatic and quasi-static process, and the gas expanded to the entire volume of the box. The temperature in the box is now T2 in equilibrium. What is T₂? (iv) Show T₁ > T₂,…A box of 10.0 cm x 10.0 cm x 10.0 cm contains 1.2 x 105 Pa of N2 gas molecules at 25°C. The mass of one N2 molecule is 4.68 x 10-26 kg and its molar mass is 28.0-g Assume all the molecules collide with the container walls with its rms speed in a head-on fashion and all the collisions are perfectly elastic, estimate the amount of molecules striking one side of the container wall in 10 seconds? (R = 8.31 J/mole/K -0.08205 Latm/mole/K, kg-1.38 X 10 23 J/K, 1 atm = 1.01X 105 Pa.) 4.1 x 1028 2.9 x 1026 3.2 x 1020 7.5 x 1022 10 x 1024 A Question 21 (4 points) Retake question I used equations in the list to solve the above problem: AT P = k₁A₁AT¹ + k2A22 + k3A3 P = KAAT AT3 L3 P = E/t P = AAT +AT+ A 1. Yes. 2. No. P=A- AT R₁+Ra+R3
- The molar specific heat at constant pressure of an ideal gas is (7/2)R. The ratio of specific heat at constant pressure to that at constant volume is (a) 7/5 (b) 8/7 (c) 5/7 (d) 9/7If one mole of a monoatomic gas of (y = 5/3) is mixed with one mole of diatomic gas, then the (y = 715) value of y for the mixture will be, (a) 1.5 (b) 1.54 (c) 1.4 (d) 1.45An ideal gas consists of 2.50 mol of diatomic molecules that rotate but do not oscillate. The molecular diameter is 118 pm. The gas is expanded at a constant pressure of 1.79 x 105 Pa, with a transfer of 150 J as heat. What is the change in the mean free path of the molecules?
- A 1 mol sample of a diatomic ideal gas (γ=1.4) expands slowly and adiabatically from a pressure of 18 atm and a volume of 3 L to a final volume of 18 L. What is the final temprature (in K) of the gas? ( Answer no decimal )What is the average (rms) velocity of nitrogen (diatomic) gas molecules at 20 degrees Celsius?Equal moles of three different ideal gases (A, B, and C) are prepared in separate sealed chambers at different temperatures. The velocity distributions for molecules of the three gases are shown below. The gases have different molecular masses which are not known. Which of the following statements about these gases MUST BE true? Number of Molecules B C Velocity Gas C has the greatest temperature. Gas A has the greatest average kinetic energy per molecule. O Gas C has the greatest average kinetic energy per molecule. O Gas A has the greatest molecular mass. O Gas C has the greatest rms speed. Next.
- A krypton-84 atom has a mass of 1.39 x 10-25 kg. (a) What temperature (in K) would a gas composed entirely of krypton-84 atoms have to be at in order for the rms speed of the atoms to equal the escape speed from Earth, 1.12 x 10 m/s? K (b) What temperature (in K) would a gas composed entirely of krypton-84 atoms have to be at in order for the rms speed of the atoms to equal the escape speed from the Moon, 2.37 x 10 m/s? KThe temperature of 3.00 moles of argon gas is lowered from 2.50 102 K to 2.00 102 K. (a) Find the change in the internal energy, ΔU, of the gas. J(b) Find the change in the average kinetic energy per atom.If the temperature T of an ideal gas doubles, by what factor does the average kinetic energy of the atoms change?