Question

One mole of a monatomic ideal gas undergoes a reversible expansion at constant pressure, during which the entropy of the gas increases by 14.41 J/K and the gas absorbs 6236 J of thermal energy. Calculate the initial and final temperatures of the gas. One mole of a second monatomic ideal gas undergoes a reversible isothermal expansion, during which it doubles its volume, performs 1729 J of work, and increases its entropy by 5.763 J/K. Calculate the temperature at which the expansion was conducted.

Answer 1

Answer:

300K, 600K

Explanation:

ΔS =nCp ㏑($\frac{T2}{T1}$)

= (2.5) (78.314) ㏑($\frac{T2}{T1}$) = 14.41

Qp =(2.5) (8.314) (T2-T1)

      = 6236 J.

=> 20.8 (T2-T1) - 6236

=> T2-T1 = 300

=> T2=T1 + 300

20.8 ㏑($\frac{300+T1}{T1}$) = $14.41$

=> $\frac{300+T1}{T1} = 2$

=> T1 = 300K

=> T2 = 600K