Question 13 Marks
100 g of water is supercooled to -$10^\circC$. At this point, due to some disturbance mechanised or otherwise some of it suddenly freezes to ice. What will be the temperature of the resultant mixture and how much mass would freeze?
[Sw = 1cal/ $g/^\circC$ and $L^W$Fusion = 80cal/ g]
[Sw = 1cal/ $g/^\circC$ and $L^W$Fusion = 80cal/ g]
Answer
View full question & answer→Water mass = 100g At -$10^\circC$ ice and water mixture exists. Heat required (given out) by $10^\circ\text{Cice to }0^\circ\text{C ice}=\text{ms}\Delta\text{t}$$=100\times1\times[0-(-10)]$
$\text{Q}=1000\text{cal}$
Let gm ice melted Q = ml$\text{m}=\frac{\text{Q}}{\text{L}}=\frac{1000}{80}=12.5\text{g}$
So, there is m $= 12.5g$ water and ice in mixture. Hence temperature of mixture remains $0^\circC.$
$\text{Q}=1000\text{cal}$
Let gm ice melted Q = ml$\text{m}=\frac{\text{Q}}{\text{L}}=\frac{1000}{80}=12.5\text{g}$
So, there is m $= 12.5g$ water and ice in mixture. Hence temperature of mixture remains $0^\circC.$