Question

Problem 4 (10 pts) A gas cylinder with a movable piston that is filled with argon gas experiences a drop in temperature from 56.0 C to 14.2 C and the piston's leaky seal loses 0.0048 mols of its initial 0.0132 mols before getting plugged. All of this transpires under a constant pressure of 1.024 atm. (a) The initial volume of the cylinder was 13.0 L. How many calories were transferred through work? (3pts) (b) The total energy change for this process was 0.5983 kJ. How many joules of energy were transferred thermally? (3pts) (c) How many grams of Argon gas are left in the cylinder after the leak is plugged? (Ipts) (d) Use the mass from partc to calculate the specific heat capacity for argon. (3pts)

Answer 1

& Given that T = 56+ 273 = 329k T2 - 14.2 +273 - 287.2. = 13L , P = 1.024 atm V = ? Since P = constant 13 287.2 V = 1.354 @ work done at constan pressen w=PLV₂-v.) = 1.084 (11.35 - 13). [w = -lodgi cal And

ou = 0.5983 k] be - ? w - - 1.691 cal ε = -7.075 kJ from first love of thermodynamics so = BU + w = 0.5983 + (-7.075) I su = -6.47 kg Ang Initial moles = 0.0132 final Moles & moles eman = 0.0132 - 0.0048 = 0.0084 moles Amount in gram = = molex At weight 0.0084 x 40

| Amount in gram left = 0.336 game from specific heat capacity MOT a = -6.47 kJ m = 0.336 DT = T₂-T - 14.2 - 56 = – 41.8°c - – 6.47 ky 0.336X (-4118) - – 6047 x 103 0.336 (-41.8) (c = 460.66 71 kgo c/ Angi