The temperature of an ideal monatomic gas is increased from 25 C to 50 C. Does the average translational kinetic energy of each gas atom double? Explain. If your answer is no, what would the final temperature be if the average translational kinetic energy was doubled?
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The temperature of an ideal monatomic gas is increased from
25 C to 50 C. Does the average translational kinetic energy of each gas
atom double? Explain. If your answer is no, what would the final temperature
be if the average translational kinetic energy was doubled?
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- 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…A container of nitrogen molecules is at a temperature of 37.0°C. What is the mass of a nitrogen molecule in atomic mass units? [Note: nitrogen is a diatomic gas.] а. b. What is the mass of a nitrogen molecule in kilograms? C. What is the average translational kinetic energy of the nitrogen molecules? d. What is the rms speed of the nitrogen molecules? е. What is the average rotational energy of a nitrogen molecule?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.
- 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?1. The internal energy for a monatomic gas is equal to its total translational kinetic energy. 2 moles of Helium (monatomic gas, atomic mass = 4 u) are placed in a .1 m3 container and are at 60 kPa.a. Find the total translational kinetic energy?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.