Ask Question
21 September, 06:19

Ask Your Teacher A 1.04-mole sample of ammonia at 11.0 atm and 25°C in a cylinder fitted with a movable piston expands against a constant external pressure of 1.00 atm. At equilibrium, the pressure and volume of the gas are 1.00 atm and 24.2 L, respectively. (The heat capacity, CP, of ammonia at 25°C is 35.66 J·K-1·mol-1.)

(a) Calculate the final temperature of the sample.

(b) Calculate the values of q; w, and DU for the process.

+4
Answers (1)
  1. 21 September, 08:33
    0
    a) Volume of the gas nRT / P

    = 1,04 X 8.3 X 298 / 11 X 10⁵ m³

    = 233.85 x 10⁻⁵ m³

    = 233 x 10⁻² L

    2.33 L

    P₁V₁ / T₁ = P₂V₂/T₂

    (11 X 2.33) / 298 = (1 X 24.2) / T

    T = 281.37 K

    = 8.37 degree

    b) w = p x change in volume

    = 10⁵ x (24.2 - 2.33) x 10⁻³ J

    = 21.87 X 10² J

    2187 J

    q = n x Cp x (25 - 8.37)

    = 1.04 x 35.66x 16.63 J

    = 616.65 J

    ΔU = Q - W

    = 616.65 - 2187 J

    = - 1570.35 J

    =

    =
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Ask Your Teacher A 1.04-mole sample of ammonia at 11.0 atm and 25°C in a cylinder fitted with a movable piston expands against a constant ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers