Compounds like CCl2F2 are known as chloroflurocarbons, or CFCs. These compounds were once widely used as refrigerants but are now being replaced by compounds that are believed to be less harmful to the environment. The heat of vaporization of CCl2F2 is 289 J/g. How many grams of this substance must evaporate to freeze 203g of water initially at 17°C.

There are three sets of sketches below, showing the same pure molecular compound (water, molecular formula H₂O) at three different temperatures. The sketches are drawn as if a sample of water were under a microscope so powerful that individual atoms could be seen. Only one sketch in each set is correct. Use the slider to choose the correct sketch in each set. You may need the following information: melting point of H₂O: 0.0 °C boiling point of H₂O: 100.0 °C A (Choose one) (Choose one) 188. °C B 5 35. °C 4 5 (Choose one) -25. °℃

An 8.7- g ice cube is placed into 275 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water and that the ice cube has a temperature of 0 ∘C .

Calculate the mass of water that can be vaporized with 211 kJ of heat at the boiling point.

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 sample of C3H4Br2 has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for this compound is 35.4 kJ/mol. What would be the boiling temperature in °C of C3H4Br2 at a pressure of 540.0 mm Hg? Report your answer using three significant figures.

The enthalpy for boiling water is 40.7 kJ/mol. How much heat (in kJ) is required to boil 322.1 g of water?

Ice actually has negative caloric content. How much energy, in each of the following units, does your body lose from eating (and therefore melting) 67 g of ice? Heat of fusion for water is 6.02 kJ/mol. Express your answer in joules .

Dd.99.