How much energy is released to the environment by 50.0 grams of condensing water vapor? Hv = 40.7 kJ/mol
Hi @Diego, the answer to your question is 153.7kJ.
nope! Units are not consistent.
mols H2O = 50/18 = 1.83
Then
oops.Hit the wrong button.
moles H2O = grams/molar mass = 50 g/18 g/mol = 2.78
Then q = mass x delta H = 2.78 mols x 40.7 kJ/mol = 113 kJ
To find out how much energy is released by 50.0 grams of condensing water vapor, we need to use the given enthalpy of vaporization (Hv) and convert the mass of water vapor into moles.
Here's the step-by-step process:
1. Determine the molar mass of water (H2O). It consists of two hydrogen atoms with a molar mass of approximately 1 gram/mol each and one oxygen atom with a molar mass of approximately 16 grams/mol. So, the molar mass of water is 18 grams/mol.
2. Convert the mass of water vapor (50.0 grams) into moles by dividing it by the molar mass of water:
moles of water vapor = mass of water vapor / molar mass of water
= 50.0 g / 18 g/mol
≈ 2.78 mol
3. Use the enthalpy of vaporization (Hv) to calculate the energy released:
energy released = moles of water vapor × Hv
= 2.78 mol × 40.7 kJ/mol
≈ 113.13 kJ
Therefore, 50.0 grams of condensing water vapor releases approximately 113.13 kJ of energy into the environment.