Q.
2kg ice at −20∘C is mixed with 5kg water at 20∘C . Then final amount of water in the mixture would be; Given specific heat of ice =0.5cal/g∘C , specific heat of water =1cal/g∘C, Latent heat of fusion of ice =80cal/g. (in kg )
In this problem, ice will need energy to achieve the temperature of 0∘C and water will release energy to achieve the temperature of 0∘C .
Now, heat lost by 5kg water when its temperature decreases from 20∘C to 0∘C is given by Q1=msΔT=(5×(10)3)(1)(20)=105cal
And, heat required by 2kg ice when its temperature increases from −20∘C to 0∘C Q2=msΔT=(2×(10)3)(0.5)(20) =0.20×105cal
Now, the remaining energy =Q=Q1−Q2=0.8×105cal will melt some ice. Mass of ice melted is given by using the expression Q=mL ⇒m=LQ=800.8×105=1000g=1kg
Hence, the equilibrium temperature of the mixture will be 0∘C and mass of the water in equilibrium is is 5+1=6kg .