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Unformatted text preview: putting the results from 2 and 3 in equation 1, ∆Ε = q+w = 550J + 1418.2 J = 1968.2 J. 3. (6 pts) An ideal gas in a cylinder expands against a constant external pressure of 1.0 atm. from a volume of 5.0 L to a volume of 13.0 L, at constant temperature. a) Determine the initial pressure of the gas (include units). Since the external pressure is constant, the initial pressure of the gas is same as the external pressure on the gas, therefore it is 1 atm. b) Calculate the work, w (in J) associated with the expansion of the ideal gas. In isothermal expansion, W is W= -nRT ln (Vfinal / V initial) (1). n = PV/RT = c) Knowing that ∆ E = 0 for ideal gases at constant Temperature, calculate the heat flow of the system in J. Is this an endothermic or exothermic process? Since ∆ E = 0 and W < 0 as we calculated in the problem above, Q>0. Therefore, this is an endothermic process....
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- Spring '10
- Thermodynamics, Intermolecular force