Calculate the specific heat of a metal if 1,270 joules of heat were released when 256 grams of metal cooled 5.8°C. 1,890,00 g/J°C 0.855 g/J°C 1.17 g/J°C 28.8 g/J°C

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?

A piece of metal weighing 50 grams was heated to 100°C and then dropped into 250 grams of water at 25°C. The metal cooled down and the water became warmer until both were at a temperature of 28.8°C. Calculate the amount of heat absorbed by the water. Assuming that the heat lost by the copper was absorbed by the water, what is the specific heat of the metal? (sH2O = 4.18 J / g °C)

Given a 49.8-g49.8-g sample of this substance with a specific heat of 59.0 J/(kg·°C),59.0 J/(kg·°C), how much heat is required to change its temperature from 180.0 °C180.0 °C to 256.0 °C?