A 1.00-mol sample of an ideal diatomic gas is allowed to expand. This expansion is represented by the straight line from 1 to 2 in the PV diagram. The gas is then compressed isothermally. This compression is represented by the curved line from 2 to 1 in the PV diagram. Point 1 is at (11.6 L, 1.98 atm) and Point 2 is at (22.5 L, 1.00 atm) in the diagram. 2.2 Pressure (atm) 2.0 1.8 1.6 1.4 1.2 1.0 0.8 1 10 16 18 Volume (liter) Tipler & Mosca, Physics for Scientists and Engineers, 6e 2008 W.H. Freeman and Company 12 14 Calculate the work Whet per cycle done by the gas. 20 Wnet - N 22 24 2

A 1.00-mol sample of an ideal diatomic gas is allowed to expand. This expansion is represented by the straight line from 1 to 2 in the PV diagram. The gas is then compressed isothermally. This compression is represented by the curved line from 2 to 1 in the PV diagram. Point 1 is at (11.6 L, 1.98 atm) and Point 2 is at (22.5 L, 1.00 atm) in the diagram. 2.2 Pressure (atm) 2.0 1.8 1.6 1.4 1.2 1.0 0.8 1 10 16 18 Volume (liter) Tipler & Mosca, Physics for Scientists and Engineers, 6e 2008 W.H. Freeman and Company 12 14 Calculate the work Whet per cycle done by the gas. 20 Wnet - N 22 24 2

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

A gas expands from I to F in the figure below. The energy added to the gas by heat is 212 J when the gas goes from I to F along the diagonal path. Three paths are plotted on a PV diagram, which has a horizontal axis labeled V (liters), and a vertical axis labeled P (atm). The green path starts at point I (2,4), extends vertically down to point B (2,1), then extends horizontally to point F (4,1). The blue path starts at point I (2,4), and extends down and to the right to end at point F (4,1). The orange path starts at point I (2,4), extends horizontally to the right to point A (4,4), then extends vertically down to end at point F (4,1). (a) What is the change in internal energy of the gas? Use the relations between various features of the graph and the work done on the gas to find the energy added by work and then use your result to find the change in internal energy of the gas. J(b) How much energy must be added to the gas by heat for the indirect path IAF to give the same change in…
Question B: A sample of 1.00 mole of a diatomic ideal gas is initially at temperature 265 K and volume 0.200 m3. The gas first undergoes an isobaric expansion, such that its temperature increases by 110.0 K. It then undergoes an adiabatic expansion so that its final volume is 0,440 m3. i. Sketch a PV diagram for the two-step process, including labeled initial, final, and intermediate states, and a two-part curve/path with an arrow indicating direction. Label the initial state "i", the final state "f", and the intermediate state "b". Write down the known values for P, T, and V at each point, e.g. T; = 265 K, and Th = 375 K. (B.1) What is the initial pressure of the gas, Pi, in pascals [Pa]? Pi = Pa Enter a number. (B.2) What is the total heat transfer, Q, to the gas, in joules [J]? Q = Qtotal = (B.3) What is the total work done on the gas, w, in joules [J]? w = Wtotal = Enter your answer for problem (B.3) for credit. First, use the following questions as intermediate steps; answers can…
Question: 261 mols of an ideal monatomic gas undergo the process shown in the PV plot (Figure 1). The process A → B is adiabatic. In the plot below, VA 1.23 m³, VB = 3.76 m³ and PA = 3.22 atm. A A PB C VA V8 V Figure 1: A PV plot depicting the described gas going down and right from state A to state B via an adiabatic pathway. The gas then goes left from state B to state C via a horizontal pathway before going up from state C to state A via a vertical pathway. The x-axis represents volume and the y-axis represents pressure. Part 1) What is PB? PB : atm Part 2) How much heat is added as the gas goes from B → OC? QB>C J Part 3) What is AEint as the gas goes from C → A? AEint J B
An ideal gas, initially at a pressure of 9.7 ×105 Pa and a temperature of 286 K, is allowed to expand adiabatically until its volume doubles. What is the gas’s final temperature, in kelvin, if the gas is monatomic? What is the gas’s final pressure, in pascals, if the gas is diatomic?
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 =
An ideal gas is expanding isothermally from initial volume of 3.00 L at 94 atm to final volume of 24.0 L. Calculate the heat if the work is done by the gas. [1 atm: 1.013 x 105 Pa] Select one: O 0.59 J O -59402.57 J 59402.57 J O 5.9e7 J
A particular thermodynamic cycle acting on a monatomic ideal gas (y = 1.67) includes an isobaric expansion, an isochoric cooling, and then a isothermic contraction. The PV diagram is shown in the image below. P V The isobaric expansion occurs at a pressure of 1.8 × 105 Pa and changes the volume of the gas from 6.7 x 10-2 m³ to 13.08 × 102m³. What is the efficiency of the process?
A monatomic ideal gas initially fills a V0 = 0.45 m3 container at P0 = 85 kPa. The gas undergoes an isobaric expansion to V1 = 1.4 m3. Next it undergoes an isovolumetric cooling to its initial temperature T0. Finally it undergoes an isothermal compression to its initial pressure and volume. 1 Calculate the work done by the gas, W1, in kilojoules, during the isobaric expansion (first process). 2 Calculate the heat absorbed Q1, in kilojoules, during the isobaric expansion (first process). 3 Write an expression for the change in internal energy, ΔU1 during the isobaric expansion (first process). 4 Calculate the work done by the gas, W2, in kilojoules, during the isovolumetric cooling (second process). 5 Calculate the heat absorbed Q2, in kilojoules, during the isovolumetric cooling (second process). 6 Calculate the change in internal energy by the gas, ΔU2, in kilojoules, during the isovolumetric cooling (second process). 7 Calculate the work done by the gas, W3, in kilojoules,…
An ideal monatomic gas undergoes changes in pressure and volume, as shown in the pV diagram below. The initial volume is 0.02 m3 and the final volume is 0.10 m3. The initial pressure is 1 atm and the final pressure is 2 atm. Recall that 1 atm = 101.3 kPa. (a) Calculate the magnitude, or absolute value, of the work done on the gas in this process. Answer = - 13429J (c) The initial temperature of the gas is 308 K. Calculate the temperature of the gas at the end of the process. Answer = 3080 k Just need answer with the following: (d) What is the change in thermal energy for the gas in this process? (e) Calculate the quantity of heat transfer added to (positive) or removed from (negative) the gas during this process.
An expansion process on an ideal diatomic ideal gas has a linear path between the initial and final coordinates on a pV diagram. The coordinates of the initial state are: the pressure is 300 kPa, the volume is 0.700 m3, and the temperature is 390 K. The final pressure is 130 kPa and the final temperature is 310 K. How much work is done by the gas during this process? (R = 8.31 J/mol * K)
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