1. For nitrogen at 285 K find, a) The most probable speed b) The average speed c) The rms speed The molar mass of nitrogen is 14.0 g/mol and R=8.31 kg/(mol K) Hint: You need to convert quantities into Sl units. m/s m/s m/s
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- RTI The molecules in a six-particle gas have velocities ₁ (201-30j) m/s V2 (10i+60j) m/s 73=(-501 +20j) m/s 7= 30i m/s Vs (40i-40j) m/s ₁=(-50 i 10j) m/s Calculate Varg Express the x and y components of the velocity in meters per second separated by a comma. Uz avg, Uy avg Submit Part B VD|| ΑΣΦ Request Answer W Calculate Davg- Express your answer with the appropriate units. ? m/sa) Estimate the average spacing between the molecules of 1 mol of an ideal gas at a pressure of 1atm and a temperature of 300 K. b) 1 mol of liquid water occupies a volume of 18 cm. Estimate the spacing between molecules. c) Use your result from part (a) to estimate the diameter of a water molecule. d) Estimate the factor by which water expands when it boilsThe total translational kinetic energy of the molecules of a sample of gas at 455 K is 10500 J. How many moles n does the sample comprise? n = mol Find the average translational kinetic energy Kav of a single molecule. Kay = J
- What is the RMS speed of CO2 gas at a temperature of 270 C? a. 372 m/s b. 505 m/s c. 268 m/s d. 305 m/s e. 412 m/sA tank contains 16 moles of neon gas at an absolute pressure of 1 x 105 Pa. What is the change in the internal energy of the gas when the temperature is raised from 27 ºC to 32 ºC. Given: Boltzmann constant: k = 1.38 x 10–23 J/K, Ideal Gas Constant: R = 8.31 J/(mol K) 1000 J B. 750 J C. 500 J D. 250 J E. 100 JWater vapor at a pressure 0f 2X10 N/m2 0nd a dempirature of as0°c is 0.32 x106 N/m2.following expanded to a yoessune of ec.For the low P.V1.25 this expanston determine: a. Pinal vapor condnion b. Syecipie haat transpan c. Changis in tntroyy SIDU
- (a) An ideal gas occupies a volume of 1.6 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. molecules (b) If the pressure of the 1.6 cm3 volume is reduced to 1.2 ✕ 10-11 Pa (an extremely good vacuum) while the temperature remains constant, how many moles of gas remain in the container? mol example of question a An ideal gas occupies a volume of 2.4 cm3 at 20°C and atmospheric pressure. Determine the number of molecules of gas in the container. 6.01e+19 molecules2. For T = 300 K, calculate the pressure (in bars) at which the mean free path of a hydrogen molecule will be each of the lengths given here. For H₂, o = 2.30 x 10-1⁹ m². (a) 100 μm (b) 1.00 mm (c) 1.00 m LLWhich of the following statements is not true according to kinetic theory? a. The molecules in an ideal gas undergo elastic collisions. b. The molecules in an ideal gas only interact during collisions. c. Electrical attractions and repulsions between the molecules must be accounted for in the total energy of the ideal gas. d. The average energy of a molecule in an ideal gas is evenly distributed between the different degrees of freedom of the molecule. e. The energy of an ideal gas only depends on the kinetic energy of the gas.
- 8. The average energy of a mole of Einstein solid is given by: ӨЕ 3R0E Ē = 3R + 2 ӨЕ ет — 1 where E is the Einstein temperature and R the gas constant. Obtain expressions for the average energy at the limits of zero and infinite temperature and comment on your results.One mole of hydrogen has a mass of 2 g. Calculate the mean speed of the hydrogen molecules at T = 300 K using the Maxwell- Boltzmann distribution. Select one: O a. 1579 m/s O b. 1782 m/s O c. O d. 459 m/s 1934 m/sQUESTION 16 Which of the following statements is not true according to kinetic theory? a. Electrical attractions and repulsions between the molecules must be accounted for in the total energy of the ideal gas. b. The energy of an ideal gas only depends on the kinetic energy of the gas. C. The average energy of a molecule in an ideal gas is evenly distributed between the different degrees of freedom of the molecule. d. The molecules in an ideal gas undergo elastic collisions. e. The molecules in an ideal gas only interact during collisions.