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

300K, 600K

Step-by-step explanation:

ΔS =nCp ㏑(
`(T2)/(T1)`)

= (2.5) (78.314) ㏑(
`(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 ㏑(
`(300+T1)/(T1)`) =
`14.41`

=>
`(300+T1)/(T1) = 2`

=> T1 = 300K

=> T2 = 600K