One mole of H2O(g) at 1.00 atm and 100.°C occupies a volume of 30.6 L. When one mole of H2O(g) is condensed to one mole of H2O(l) at 1.00 atm and 100.°C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate E for the condensation of one mole of water at 1.00 atm and 100.°C.

Delta E = q + w

q = -40.66 kJ.
w = -p(delta V) = -p(V2-V1)
p = 1.00 atm.
V1 = 30.6 L
V2 = calculated from density. 1 mol H2O has mass of 18.015 g, density is 0.996, V2 = ??
Don't forget to change w from L*atm units to J by multiplying w*101.3 J/L*atm. Also remember w is in Joules and q is in kJ so make them the same unit.

Post your work if you get stuck.

i don't get how to convert the density to V2...

density=mass/volume so volume=mass/density

how do you convert cm^3 to L so you can subtract V1 from V2

100 Cm^3=1 L

1000 cm^3 = 1 L since 1 cm^3 = 1 mL and since there are 1000 mL in one L.

To calculate the energy (E) for the condensation of one mole of water at 1.00 atm and 100.°C, we can use the formula:

E = q / n

Where:
E = Energy
q = Heat released
n = Number of moles of substance

From the given information, we know that 40.66 kJ of heat is released when one mole of H2O(g) is condensed to H2O(l). So, q = -40.66 kJ (negative sign because heat is released).

We also know that one mole of H2O(g) occupies a volume of 30.6 L at 1.00 atm and 100.°C.

Now, we can calculate the number of moles (n) of water using the ideal gas law:

PV = nRT

Where:
P = Pressure
V = Volume
R = Ideal gas constant (0.0821 L.atm/mol.K)
T = Temperature

Rearranging the equation, we have:

n = PV / RT

Substituting the given values, we have:

n = (1.00 atm * 30.6 L) / (0.0821 L.atm/mol.K * 373 K)

Simplifying the equation further, we have:

n = 1.00 mol

Now, we can substitute the values of q and n into the formula for energy:

E = (-40.66 kJ) / (1.00 mol)

Calculating this, we find:

E = -40.66 kJ/mol

Therefore, the energy for the condensation of one mole of water at 1.00 atm and 100.°C is approximately -40.66 kJ/mol.