The entropy change when an ideal gas under atmospheric condition at room temperature is allowed to expand from text0 text.5 textL to text1 text.0 textL and also is simultaneously heated to text373 textK will be (Given: textC textv, textm text= text12 text.50 J K- text1 textmol- text1 and textlog text1 text.25 text= text0 text.1 )

Question

The entropy change when an ideal gas under atmospheric condition at room temperature is allowed to expand from text0 text.5 textL to text1 text.0 textL and also is simultaneously heated to text373 textK will be (Given: textC textv, textm text= text12 text.50 J K- text1 textmol- text1 and textlog text1 text.25 text= text0 text.1 ) (A)  text0.18 J textK- 1 (B)  text0.36 J textK- 1 (C)  text0.90 J textK- 1 (D)  text0.72 J textK- 1

Tardigrade Admin · Accepted Answer

n=(P V/R T)=0.02 moles textÎS text= textnRln ( textV text2/ textV text1) + textnC textv,m textln ( textT text2/ textT text1) textÎS text= text0 text.12 text+ text0 text.06 textÎS text= text0 text.18 textJK- 1

Q. The entropy change when an ideal gas under atmospheric condition at room temperature is allowed to expand from $0 .5 L$ to $1 .0 L$ and also is simultaneously heated to $373 K$ will be

(Given: $C_{v, m} = 12 .50 J K^{- 1} mol^{- 1}$ and $log 1 .25 = 0 .1$ )

$0.18 J K^{- 1}$

$0.36 J K^{- 1}$

$0.90 J K^{- 1}$

$0.72 J K^{- 1}$

$n = \frac{P V}{RT} = 0.02$ moles

$ΔS = nRln \frac{V _{2}}{V _{1}} + nC_{v,m} ln \frac{T _{2}}{T _{1}}$

$ΔS = 0 .12 + 0 .06$

$ΔS = 0 .18 JK^{- 1}$

Q. The entropy change when an ideal gas under atmospheric condition at room temperature is allowed to expand from 0.5L to 1.0L and also is simultaneously heated to 373K will be (Given: Cv,m​=12.50 J K−1mol−1 and log1.25=0.1 )

0.18 J K−1

0.36 J K−1

0.90 J K−1

0.72 J K−1