For many years drinking water has been cooled in hot climates by evaporating it from the surfaces of canvas bags or porous clay pots. How many grams of water can be cooled from 44 ∘C∘C to 25 ∘C∘C by the evaporation of 52 gg of water? (The heat of vaporization of water in this temperature range is 2.4 kJ/gkJ/g. The specific heat of water is 4.18 J/g⋅KJ/g⋅K.)

thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J·g *.°C*, is put into a calorimeter (see sketch at right) that insulated container contains 100.0 g of water. The aluminum sample starts off at 91.4 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. water Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. sample a calorimeter x10

An 19.5-g ice cube at 0 ∘C is placed onto a 245-g block of aluminum. Calculate the temperature change of the aluminum upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from aluminum. The specific heat capacity of aluminum is 0.903 J/g ∘C and the heat of fusion for water is 6.02 kJ/mol. Express the temperature change in degrees Celsius to three significant figures.    please do with complete detail explanation please

A 47.0-g sample of copper at 99.3 °C is dropped into a beaker containing 158 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g ⋅ K and 0.385 J/g ⋅ K, respectively.)

Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C

A patient arrives in the emergency room with a burn caused by steam. Calculate the heat that is released when 16.2 g of steam at 100. ∘C hits the skin, condenses, and cools to body temperature of 37.0 ∘C. (For water, 540 cal (2260 J) is needed to convert 1 g of water to vapor at 100 ∘C.)

If 31.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The ∆H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g°C), and that no heat is gained or lost by the container, what will be the final temperature of the solution?

How many grams of water would require 2,247 joules of heat to raise its temperature from 36.86 °C to 100°C?

If 3.00 kJ of heat is supplied to a 0.880 mol sample of solid copper at 25.0°C, what will the copper’s final temperature be in °C? (The specific heat of solid copper is 0.385 J/g • K.)

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.