Question

A 2.00 mol sample of a diatomic ideal gas expands slowly and adiabatically from a pressure of 5.04 atm and a volume of L2 Lto a final volume of 30.8 L (a) What is the final pressure of the gas? 1.44 atm (b) What are the initial and final temperatures? initial 385.72 final 269.39 (c) Find Qfor the gas during this process. 0 (d) Find ??¡nt for the gas during this process. What is the relationship between the internal energy and the temperature of an ideal gas? k (e) Find W for the gas during this process. Enter a number work is defined as the work done on the gas. kJ Need Help? ReadliMaster M Read It Master It Submit Answer Save Progress Practice Another Version

Answer 1

Q = 0 so delta(E_int) = - W

and for adiabatic process,

W = (P1 V1^Y)[ V2^(1-Y) - V1^(1-Y)] / (1 - Y)

P1 = 5.04 x 101325 Pa

V1 = 12.6 x 10^-3 m^3

and V2 = 30.8 x 10^-3 m^3

for diatomic, Y = 7/5 = 1.40

putting values,

W = 4835.5 J

(D) delta(E_int) = - 4835.5 J

(E) W = 4835.5 J