A sample of steam with a mass of 0.529 g at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °c. (For water, AHvap = 40.7 kJ/mol and Cwater = 4.18 J/(g · °C).) - Part A Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using three significant figures.

The heat absorbed or liberated by a substance (q) can be calculated using the following equation: q = g C ΔT, where g is the mass in grams, C is the heat capacity per unit mass, and ΔT is the change in temperature. Use the following values to calculate the energy required to convert one gram of ice at 0°C to one gram of steam at 100°C. The heat capacity of water is 4.25 J/g °C. The heat of fusion (the amount of heat required to change a solid into a liquid at its melting point) of ice is 335 J/g. The heat of vaporization of water is 2258 J/g.

A sample of 3.20 g of calcium hydroxide, Ca(OH)2(s) is added to 90.0 mL of dilute hydrochloric acid in a calorimeter.  The temperature goes from 22.4°C to 24.7°C.  Calculate the molar enthalpy of the reaction?

Energy Constants for H2O334 J/g = Heat of Fusion (Hf)2260 J/g = Heat of Vaporization (Hv)2.11 J/goC = Specific Heat Capacity of solid water4.18 J/goC = Specific Heat Capacity of liquid water2.00 =J/goC = Specific Heat Capacity of water vapor3.  A 12-oz can of soft drink (m = 340 g) at 25oC is placed in a cooler where the temperature is 0oC.  How much energy must be removed from the soft drink for it to become ice at 0oC?