1. The formation of condensation on a glass of ice water causes the ice to melt faster than it would otherwise. If 7.10 g of condensation forms on a glass containing water and 230 g of ice, how many grams will melt as a result? Assume no other heat transfer occurs. Use the heat of vaporization of water at 37°, as an approximation, in this problem.

1. Two 50g ice cubes are dropped into 200g of water in a thermally insulated container. The water is initially at 25°C, and the ice comes directly from a freeze at -15°C, what is the final temperature of the drink when the drink reached thermal equilibrium?

8. You drop 182 g of ice at 0°C into a glass containing 431 ml of water at a temperature of 28°C. How many grams of ice will be remaining once the temperature has attained a steady-state (i.e. once it has stopped changing)? Ignore the effects of the glass. Quantity Specific Heat Capacity of Liquid Water 4190 J/kg/°C Specific Heat Capacity of Ice Value 2100 J/kg/°C 334 x 10 J/kg 1 g/ml Latent Heat of Fusion of Water Density of Liquid Water About 31 g About 151 g About 34 g About 65 g About 249 g

10. In an experiment to determine the specific heat capacity of a certain metal, a student obtained the values given below; Mass of water Mw = 44.3g Mass of calorimeter, Mc = 58.7g Initial temperature of water before boiling, T₂= 18.4 °C Final temperature reached by the heated water, T₁= 85.4 °C Final temperature reached by the mixture (water+ calorimeter+ specimen metal), TF = 20.2 °C Calculate the specific heat capacity, C₁ of the specimen metal using the equation; C₁= {[(MwCw+McCc) (TF-T2)] / M1(T1-TF)} Where; specific heat capacity of water, Cw=4186J/Kg K - specific heat capacity of the calorimeter, Cc= 386J/Kg K Mass of the specimen, M₁ = 17.4g