Problem 2: Atmospheric compositionA particle near earth's surface traveling faster than about 11km/s has enough kineticenergy to completely escape from the earth, despite earth's gravitational pull. Moleculesin the upper atmosphere that are moving faster than this will therefore escape if they donot collide on the way out.a) The temperature of earth’s upper atmosphere is actually quite high, around 1000K.Calculate the probability of a nitrogen molecule at this temperature moving fasterthan 11km/s, and comment on the result.b) Repeat the calculation for a hydrogen molecule (H2) and for a helium atom, anddiscuss the implications.c) Escape speed from the moon's surface is only about 2.4km/s. Explain why themoon has no atmosphere.

Part(a) Basic Details The equation for the probability for any particle from the earth’s atmosphere…

Answered: Problem 2: Atmospheric composition A…

Similar questions

#4 and #5 questions. Thank you! Initial Particle 60 Temperature 300 K avg. speed 465 m/s Initial pressure 7.1 atm Final Particle 160 Temperature 300 K avg. speed 455 m/s final pressure 18.6 atm
A sample of a monatomic ideal gas initially at temperature T, undergoes a process during which the pressure of the gas triples and its volume also triples. What is the change in the temperature (AT) of the gas, in Kelvins? A. T B. 8T C.9T D. 7/9 E. T18 OB O O O DA OE
P4
2 Thermo Physics The ground state of Cyanogen gas (Energy = 0 eV) and 1st excited state is (E = 4.7x10^-4eV) can be separately identified by their spectra. An astronomer determines that on interstellar gas has a ratio of 10:1. 10 molecules of cyanogen gas to every 1 excited state. Use this to determine the temperature of the gas?
5
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.
Learning Goal: To understand the ideal gas law and be able to apply it to a wide variety of situations. The absolute temperature T, volume V, and pressure p of a gas sample are related by the ideal gas law, which states that PV = nRT Here n is the number of moles in the gas sample and R is a gas constant that applies to all gases. This empirical law describes gases well only if they are sufficiently dilute and at a sufficiently high temperature that they are not on the verge of condensing. In applying the ideal gas law, p must be the absolute pressure, measured with respect to vacuum and not with respect to atmospheric pressure, and I must be the absolute temperature, measured in kelvins (that is, with respect to absolute zero, defined throughout this tutorial as -273°C). If p is in pascals and V is in cubic meters, use R = 8.3145 J/(mol · K). If p is in atmospheres and V is in liters, use R = 0.08206 L atm/(mol-K) instead. Part A A gas sample enclosed in a rigid metal container at…
V₁₂: V₁ = 4:1 V₁ V₂ There are 6 molecules of a gas in V₂ and none in V₁. Now a hole i made in partition. Find the probability of finding 3 molecules on each side of the partition.
8
a. Explain what the temperature of an ideal gas actually measures, molecularly b. You have two containers, the first with 1 mole of helium and the second with 5 moles of neon at the same temperature. Which gas has more thermal energy? Explain.
2.00 mol of helium and 1.00 mol of argon are separated by a very thin barrier. Initially the helium has 7500 J of thermal energy. The helium gains 2500 J of energy as the gases interact and come to thermal equilibrium by exchanging energy via collisions at the boundary. What was the initial temperature of the argon? First, what is the equilibrium temperature of the two gases? Express your answer in kelvins. ► View Available Hint(s) Tf = Submit Part B VE ΑΣΦ help What is the thermal energy of the argon at the equilibrium temperature? Express your answer with the appropriate units.
A tank of N2 gas has temperature 500 K. Calculate the percentation of N2 molecules that has a speed between 1000 m/s and 2000 m/s. ____% 2 sig. fig. Please solve in Excel numerically the Maxwell-Boltzmann distribution

SEE MORE QUESTIONS