A cylinder with a piston contains 0.250 mol of oxygen at 2.40 * 10^5 Pa and 355 K. The oxygen may be treated as an ideal gas. The gas first expands isobarically to twice its original volume. It is then compressed isothermally back to its original volume, and finally it is cooled isochorically to its original pressure. Compute the maximum pressure

Two containers each hold 1 mole of an ideal gas at 1 atm. Container A holds a monatomic gas and container B holds a diatomic gas. The volume of each container is halved while the pressure is held constant. (Assume the initial volumes of containers A and B are equal.) (c) What is the ratio  QA QB  of the energy transferred to gases A and B?

A sample of n = 2.00 moles of monoatomic ideal gas expands adiabatically, the work done on the gas is W = -5.00 x 103 J.  The initial temperature and pressure of the gas are   Ti = 600 K and Pi = 4.05 x 105 Pa.  Calculate: a) the final temperature of the gas; b) the final pressure of the gas.  R = 8.314 J/mol K

A container having a volume of 2.30 L holds 1.80 g of helium gas at a temperature of 29.0 °C. (a) Find the pressure in the container. P = atm (b) Helium behaves as an ideal monoatomic gas. Find the internal energy of the system. Eint =

5kg on it which can slide up and A cylinder with an ideal gas has a piston of mass m = down and does not permit the gas to escape. The inner radius of the cylinder is r = 6cm, The top of the piston is open to atmospheric pressure. The entire system is initially in thermal equilibrium with the environment, which is at 20°C and the height of the piston h = 10cm. If the temperature of the gas inside then is raised to 100°C, what is the final height of the piston? A 20 cm В 50 cm C 12.7 cm D 25.4 cm 18 cm Open to outside air, pressure po Piston, mass m Ideal- gas

A student decides to conduct an experiment by using two different flasks and two different gas samples. In flask 1, there exists Neon (Ne) gas, whereas the second flask is filled with nitrogen (N2) gas. If both flasks are kept at 270 K, answer the following questions. (Note: Molar mass of N2 = 28.014 g mol1,molar mass of Neon = 20.1797 g mol, R= 8.31 J. mol1.K1, k=1.38 x 1023 J.K-1, Avogadro's number = 6.02 x 1023 mol1.) a) Find the average kinetic energy of one Neon molecule. b) Calculate the average kinetic energy (translational+rotational) of one nitrogen molecule by including rotational motion in your calculations. c) Find the root-mean-square speed of one neon molecule. V ms1 Check

An ideal diatomic gas undergoes an adiabatic compression during which time its volume changes from VA = 1300 cm3 to VB = 390 cm3. If its initial temperature is TA = 74.0°C, what is the final temperature TB of the gas?

A sealed ideal gas system contains 2.0 moles of monatomic ideal gas, initially at temperature 300 K and pressure 1.2 atm. The system is allowed to expand isothermally to five times its original volume. How much heat is transferred into the system during this process? 7.09 kJ 11.2 kJ 8.03 kJ Zero 4.97 kJ

A monatomic ideal gas initially fills a container of volume V = 0.25 m3 at an initial pressure of P = 390 kPa and temperature T = 325 K. The gas undergoes an isobaric expansion to V2 = 0.75 m3 and then an isovolumetric heating to P2 = 780 kPa. Calculate the number of moles, n, contained in this ideal gas.  Calculate the temperature of the gas, in kelvins, after it undergoes the isobaric expansion.  Calculate the change in entropy of the gas, in kilojoules per kelvin, as the material undergoes the isobaric expansion.