I got parts a,b, and c correct. I need help with both questions d and e. Please
ID: 716427 • Letter: I
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I got parts a,b, and c correct. I need help with both questions d and e. Please give step by step answers so I am able to follow the logic. Thank you!
1. S7 points I Previous Answers My Notes Assuming the gases in this problem are ideal. A cylinder containing some gas A is fitted with an idealized piston. Gas A is at 12.0 atm, 10.0 L and at 498K a)The gas is allowed to expand isothermally against a constant external pressure of 3.80 atm until equilibrium is reached. Compute: i) amount of A, na 2935 moles i) the new volume, VA 31.58 ii) the work done, w -8.309 k b) The gas undergoes the expansion process as described in part a and arrives at the same final state, but the process this time is done isothermally and reversibly. What is w? -14.16 K c) If w were a state function, the work computed in part a would be the same as the work computed in part b. d) Now after arriving at this state, another gas B is introduced, while thermal equilibrium is maintained. If the mole fraction of B is 0.34, to what volume must it isothermally expand to remain in equilibrium with the external pressure of 3.80 atm? e)How much work is done to expand to this volume if it does so irreversibly? (Report each to three significant figures.) L? KJ?Explanation / Answer
According to Avogadro's law, at identical condition of temperature and pressure, equal volume of gases contain equal no. of molecules. Since here, the temperature (due to thermal equilibrium) and pressure remains the same, the volume will increase proportional to increase in the no. of mopecumol. Since the mole fraction of B is 0.34, we know that the mole fraction of A is 1 - 0.34 = 0.66; we know that no. of moles of A is 2.935, therefore the total no. of moles = 2.935/0.66. We see that the no. of moles in the container increased by a factor of 1/0.66, therefore the volume will also increase by the same factor. Thus the new volume is 31.58/0.66 = 47.84L
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