How many KJ are released when 75.0g of steam at 100 degree C condenses cools to 0 degree C and freezes at 0 degree C?

I set it up like this but it is wrong,
What am I doing wrong:
75g x 2260J/1g water x 1Kj/1000J =

To calculate the amount of energy released when steam condenses and cools to 0 degrees Celsius, and then freezes at 0 degrees Celsius, you need to consider two processes.

First, you need to calculate the energy released when the steam condenses and cools from 100 degrees Celsius to 0 degrees Celsius. This can be done by using the formula:

q = m * ΔH

where q is the heat energy, m is the mass of the substance (in grams), and ΔH is the enthalpy change.

For water, the enthalpy change from steam to liquid at 100 degrees Celsius is 40.7 kJ/mol. However, we need to convert grams to moles to use this value. The molar mass of water is approximately 18.02 g/mol, so we can calculate the number of moles:

moles = mass / molar mass
moles = 75g / 18.02 g/mol ≈ 4.16 mol

Now, we can calculate the energy released when the steam condenses and cools:

q1 = moles * ΔH
q1 = 4.16 mol * 40.7 kJ/mol = 169.35 kJ

Next, we need to calculate the energy released when the liquid water freezes from 0 degrees Celsius to 0 degrees Celsius (since freezing is an exothermic process). The enthalpy change for freezing water is -6.01 kJ/mol. Again, we convert grams to moles:

moles = mass / molar mass
moles = 75g / 18.02 g/mol ≈ 4.16 mol

Now, we can calculate the energy released when the liquid water freezes:

q2 = moles * ΔH
q2 = 4.16 mol * -6.01 kJ/mol = -24.28 kJ

Finally, we can calculate the total energy released by summing the two energy contributions:

Total energy released = q1 + q2
Total energy released = 169.35 kJ + (-24.28 kJ) = 145.07 kJ

Therefore, the total energy released when 75.0g of steam at 100 degrees Celsius condenses, cools to 0 degrees Celsius, and freezes at 0 degrees Celsius is approximately 145.07 kJ.