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)

For a planet to have an atmosphere, gravity must be sufficient to keep the gas from escaping The escape speed a particle needs to escape the earth's gravitational attraction is 1.1 x 10 m/s. The motion of projectiles never depends on mass, so this escape speed applies equally to rockets and to molecules in the earth's upper atmosphere. Part A At what temperature does the rms speed of nitrogen molecules equal the escape speed? Express your answer in kelvins. ΜΕ ΑΣΦΑ T- Submit Part B T- Request An At what temperature does the mms speed of hydrogen molecules equal the escape speed? Express your answer in kelvins. VAZO Submit ? K K

So each four dot shows four different states for an ideal gas. P is the pressure and the other one is the density of the gas. Is temperature of state 1 less or greater than the state 2? Can you please explain why?

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…

Problem #1: An ideal gas of initial volume V=1m^3, initial temperature T=1000C and initial pressure P=10,000 Pa is heated up to a final temperature T=3000C and allowed to expand into a final volume V=3m^3. What is the final pressure?

A 2100 cm^3 container holds 0.15 mol of helium gas at 330C. 1. How much work must be done to compress the gas to 1400cm^3 at constant pressure?  2. How much work must be done to compress the gas to 1400cm^3 at constant temperature?

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.

The enthalpy of 36 g of water vapor increases by 1830 J when its temperature increases from 150C to 175C. Assume that water vapor is an ideal gas. 1. What is the molar specific heat at constant pressure in SI units for water vapor? 2. By how much did the water vapor’s thermal energy increase? 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