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You have 1.45 kg of water at 27.4°C in an insulated container of negligible mass. You...

You have 1.45 kg of water at 27.4°C in an insulated container of negligible mass. You add 0.680 kg of ice that is initially at -22.4°C. Assume no heat is lost to the surroundings and the mixture eventually reaches thermal equilibrium. If all of the ice has melted, what is the final temperature (in °C, round to 2 decimal places) of the water in the container? Otherwise if some ice remains, what is the mass of ice (in kg, round to 3 decimal places) that remains?

NB. Lf,ice = 3.34 x 105 J/kg , cwater = 4190 J/kg·K , cice = 2100 J/kg·K

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