Any help with this Physics question would be much appreciated.?

Specific heat of ice = 0.5 cal/gm°C

Latent heat of ice = 80 cal/gm

Specific heat of water = 1.0 cal/gm°C

The energy absorbed by the ice as it melts and the water warms will equal the energy lost by the liquid water and container as they cool. The net energy exchange is zero.

Let the final temperature be T in °C

First let's check to see if all the ice melts and assume the final temperate is 0°C

The energy given up by the liquid water and container is

E = 210(1.0(13.8 - 0) + 106(0.200)(26.7 - 0) = 3464 calories

the energy needed to warm the ice to completely melted is

E = 52.5((0.5)(0 - (-11.1)) + 80) = 4491.375

As the original liquid and container do not give up as much energy as the Ice needs to melt, the final temperature cannot be above 0°C

The Energy needed to bring the ice to melting temperature of 0° C is

E = 52.5(0.5)(0 - (-11.1)) = 291.375 calories

As the originally liquid water and container give up more than this amount and less than that needed to completely melt the ice, the final temperature must be 0°C

I hope this helps.

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