Question

A vessel of mass 100 g (S.H.C. = 0.2 calg⁻¹°C⁻¹) contains 500 g of water at 37°C. Calculate the amount of ice, which should be added to the vessel, so that the final temperature is 17°C.

[S.H.C. of water = 1 calg⁻¹°C⁻¹ and S.L.H. of ice = 80 cal g⁻¹]

Answer 1

Let the mass of ice be x g.

Heat gained by ice = 80x + 17x = 97x cal

Heat lost by water = 500 × 1 × (37 − 17) = 10000 cal

Heat lost by vessel = 100 × 0.2 × (37 − 17) = 400 cal

Total heat lost = 10000 + 400 = 10400 cal

Heat gained = Heat lost

97x = 10400

x = \[\frac{10400}{97}\]

x = 107.2 g