0.10 L of water is slowly heated from 27 ℃ to 87 ℃. What is the change in entropy?
we knew given that
T1=273+27=300 K
T2=273+87=360K
m =density x volume
m= 0.1 x 1 =0.1 Kg
Change in entropy,
dS =m Cp In(T2/T1)
dS =0.1x4186 x In(360/300 dS =76.31 J/K
0.12 L of water is slowly heated from 26 °C to 88 °C. What is the change in entropy?
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