Compounds like CCl2F2 are known as chlorofluorocarbons, 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. What mass of this substance must evaporate to freeze 195 g of water initially at 17°C? (The heat of fusion of water is 334 J/g; the specific heat of water is 4.18 J/g-K.)

i got 270g but its wrong. caus esomeone please show me the work

If you will show your work I will find the error.

To solve this problem, we need to calculate the amount of heat needed to freeze the water and compare it with the heat of vaporization of CCl2F2.

First, let's calculate the amount of heat needed to freeze the water:

1. Determine the change in temperature of the water.
- The water is initially at 17°C and will freeze at 0°C, so the change in temperature is: ΔT = 0°C - 17°C = -17°C.

2. Calculate the heat required to freeze the water using the equation:
q = m * ΔHf
where q is the heat, m is the mass, and ΔHf is the heat of fusion of water.
- The mass of water is given as 195 grams.
- The heat of fusion of water is given as 334 J/g.
- Substitute these values into the equation: q = 195 g * 334 J/g = 65130 J.

Now, let's compare this heat with the heat of vaporization of CCl2F2:

3. Determine the amount of CCl2F2 required to release the same amount of heat.
- The heat of vaporization of CCl2F2 is given as 289 J/g.
- Divide the heat required to freeze the water (65130 J) by the heat of vaporization of CCl2F2 (289 J/g): 65130 J / 289 J/g ≈ 225.28 g.

Therefore, the mass of CCl2F2 that must evaporate to freeze 195 g of water initially at 17°C is approximately 225.28 grams.