By a hot summer day, you want to serve some refreshments to your friends. To each glass, if you pore 200.0 mL of cold tea at 20.0°C and add 10 ice cubes at – 10.0°C each weighing 10.0 g. When you measure the temperature of a glass of tea, you find that the final temperature is 0.0° How much heat did the ice cubes gain to reach that temperature. Will the entire ice melt? If not, how much ice will melt?   Useful data:     Density of ice tea: ~ 1.00 g/mL                         C (ice tea) = 4.12 J/g.°C                         C (ice) = 2.11 J/g.°C                         DH = 6.02 kJ/mol

A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(g·°C)?0.385 J/(g·°C)? Assume no heat is lost to surroundings.

4. An ice cube at a temperature of -4.0°C has a mass of 7.0 g. You add 150. mL of hot water (90.0°C) to the ice cube. The water cools to 50.00°C. Calculate the heat of fusion (Q) in kJ and the enthalpy of fusion (AH) in kJ/mol.

thermometer A 58.2 g sample of polystyrene is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The polystyrene insulated container sample starts off at 89.1 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 23.0 °C. The pressure remains constant at 1 atm. water Calculate the specific heat capacity of polystyrene according to this experiment. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter J Ox10 g.°C ?

How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

A 54.5 g sample of brass is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The brass sample starts off at 95.8 °C and the temperature of the water starts off at 15.0 °C. When the temperature of the water stops changing it's 16.4 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of brass according to this experiment. Be sure your answer is rounded to 2 significant digits. П J g.°C x10 X S thermometer insulated container water sample a calorimeter U!!! 0 C

A 135.0-g piece of iron is heated to 225 ℃ in an oven.  It is then dropped into a calorimeter containing 250.0-mL of glycerol (d = 1.261 g/mL) at 23.5 ℃.  The temperature of glycerol rises to a maximum value of 44.7 ℃.  Determine the specific heat of glycerol.

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 15.2 g, and its initial temperature is −13.9 ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.9⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. Constants for water can be found in this table.   Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H 2 O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) *  Specific heat of liquid H 2 O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) *  Specific heat of gaseous H 2 O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) *