Question

Question 16 (1 point) Saved Two moles of an ideal gas does 3600 J of work on its surroundings as it expands isothermally to a final pressure of 1.00 atm and a volume of 46.0 L. Determine (a) the initial volume and (b) the temperature of the gas. (a) 10.4 L; (b) 2.77° C (a) 11.2 L; (b) 6.86° C (a) 21.2 L; (b) 6.86° C (a) 10.4 L; (b) 27.7°C (a) 21.2 L; (b) 68.6° C

Answer 1

Given data Number of moles of the gas n = 2 Work done by the W = 3600J gas 4 Eint Change in internal energy = 0 = 0 (expands isothermally). Final Pressure of the Pf = 1 X 1.013X10S pa gas Final volume of the Vf = (46x810-3) m3 gas on the Since the gas expands isothermally, the work done gas is found from W = nRT Inc HRT in lees) Take the exponential of both sides eW/URT Vi VE Vi = Vf.e What Substitute Pfert for WRT PV. NRT Vi = Vf. e W/ Pf vf Putting the values vi = (46X10-3).e - 3600 (1.013X10 5) (46X10-3) 0.0212 44 m3 21:2L

62 Tz Pv=nRT Pf Vf=URT Pf vf UR (1.013X105) (46X10-3) T = 2 X 8.314 280.23 K -(280.23 - 273,15 ) °c = 07.08°C یہ دعووه 6.86°c