Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • Engineering
  • At ideal gas expands internally from It to <img alt="\mathrm{2 t}"

At 300\: \mathrm{K\: cm} ideal gas expands internally from It to \mathrm{2 t} against a constant pressure of \mathrm{1.5 \mathrm{~atm}}. What is the change in enthalpy of Surroundings if the gas was \mathrm{1 mol\: in \, \mathrm{JK}^{-1}} \mathrm{(1L\: atm =101.3 \mathrm{~J} )} and the expansion is isothermal.
 

Option: 1

-0.5 \mathrm{JK}^{-1}
 


Option: 2

\mathrm{-2\: J K^{-1}}
 


Option: 3

\mathrm{+1 J K^{-1}}
 


Option: 4

\mathrm{+0.5 \mathrm{JK}^{-1}}


Answers (1)

best_answer

For isothermal \mathrm{\triangle H=O}

\mathrm{9 =-\omega=P_e \times \Delta H }

    \mathrm{=1.5(2-1) }

   \mathrm{=1.5\: \mathrm{L\: atm} }

\mathrm{=-1.5 \times 101.3 \mathrm{~J}=\text { Heat released } }

\mathrm{ \Delta S =\frac{-1.5 \times 101.3}{300}=-0.5065 \mathrm{JK}^{-1}}

Hence option 1 is correct.






 

Posted by

seema garhwal

View full answer

JEE Main high-scoring chapters and topics

Study 40% syllabus and score up to 100% marks in JEE

Similar Questions

Latest Question