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.

Explanation:

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

=

=

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.