3.14 2.5 moles of a monatomic ideal gas is initially at T = 300 K andP = 1.0 atm. The gas is then taken on a three-step cycle: (i) The pressureand volume increase in such a way that P is proportional to V, untilP = 2.0 atm; (ii) pressure is reduced at constant volume to 1.0 atm; and(iii) volume is reduced at constant pressure until the initial state isreached. (a) Find the internal energy and volume occupied by the gasin its initial state. (b) Find AU, W, and Q for each step in the process.(c) Find the net values of AU, W, and Q for the entire cycle. (d) Explainwhy the signs on your answers in (c) make sense.

Answered: Image /qna-images/answer/bdc1348a-5724-4d0c-8d28-50189cfb58c8.jpg

Answered: 3.14 2.5 moles of a monatomic ideal gas…

Similar questions

Suppose a monatomic ideal gas is changed from state A to state D by one of the processes shown on the PV diagram. PA Isotherms P₂2 atm P₁ atm A kJ E IN T B C 1 1 L I 4.00L 8.00L 16.0L V where P₁ = 1.10 and P₂ = 2.20. mat is the total work done on the gas if it follows the constant-temperature path AC followed by the constant-pressure path CD?
An ideal gas initially at 340 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 12.6 kJ is transferred to the gas by heat. (a) What is the change in internal energy of the gas? kJ (b) What is the final temperature of the gas? K
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 cylinder containing n mol of an ideal gas undergoes an adibatic process. Starting with dW = pdV and using the condition pVY = constant, show that the work done by the gas: 1 W × (p;V; - PfV¢) %3D Starting from the first law of thermodynamics in differential form, prove that the work done by the gas is n×Cy(T; - Tf).
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 3.65-mol sample of an ideal diatomic gas expands adiabatically from a volume of 0.1210 m3 to 0.750 m3. Initially the pressure was 1.00 atm. Determine: (a) the initial and final temperatures; (b) the change in internal energy; (c) the heat lost by the gas; (d) the work done on the gas. (Assume no molecular vibration.)
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
An ideal monatomic gas expands isothermally from 0.570 m³ to 1.25 m³ at a constant temperature of 800 K. If the initial pressure is 1.18 x 105 Pa find the following. (a) the work done on the gas (b) the thermal energy transfer Q J (c) the change in the internal energy J
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.