H2O (liquid) yields H2O gas delta H= +44kJ.

How much heat is evolved when 9.0 grams of water vapor is condensed to liquid water?

Well, when water vapor condenses to liquid water, it releases heat. So, it's like a steamy breakup. And according to the given information, the heat of vaporization for water is +44 kJ.

To find out how much heat is evolved when 9.0 grams of water vapor condenses, we need to use a bit of stoichiometry.

First, let's convert 9.0 grams of water vapor to moles. The molar mass of water is approximately 18 grams/mole, so 9.0 grams is equal to 0.5 moles.

Since the molar ratio between water vapor and liquid water is 1:1, we can say that 0.5 moles of water vapor will produce 0.5 moles of liquid water.

Now, we can multiply the number of moles of water (0.5 moles) by the heat of vaporization (+44 kJ) to get the amount of heat evolved.

0.5 moles * +44 kJ/mole = +22 kJ

So, when 9.0 grams of water vapor is condensed to liquid water, approximately +22 kJ of heat is evolved. And that's the tale of a steamy breakup!

To find the amount of heat evolved when 9.0 g of water vapor is condensed to liquid water, we need to use the heat of vaporization for water.

The given value, delta H = +44 kJ, represents the heat of vaporization, which is the amount of energy needed to convert 1 mole of liquid water into water vapor.

To solve this problem, we can follow these steps:

Step 1: Calculate the number of moles of water vapor.
We know that the molar mass of water (H2O) is approximately 18.015 g/mol. To find the number of moles, we divide the mass (9.0 g) by the molar mass:

Number of moles = mass / molar mass = 9.0 g / 18.015 g/mol ≈ 0.499 moles

Step 2: Determine the amount of heat evolved.
Since the heat of vaporization given is for 1 mole of water, we can use the molar ratio between water vapor and the heat evolved:

Heat evolved = delta H × number of moles = +44 kJ/mol × 0.499 moles ≈ +21.956 kJ

Therefore, approximately 21.956 kJ of heat is evolved when 9.0 grams of water vapor is condensed to liquid water.

To find out how much heat is evolved when water vapor is condensed to liquid water, we can use the concept of molar enthalpy. Molar enthalpy is the heat change that occurs when one mole of a substance undergoes a specific change.

In this case, we are given the enthalpy change (ΔH) for one mole of water vapor (H2O gas) condensing to liquid water. The given value is ΔH = +44 kJ.

To solve this problem, we need to find the number of moles of water vapor in 9.0 grams. To do this, we can use the molar mass of water, which is approximately 18.0 grams per mole.

First, calculate the number of moles of water vapor:

Number of moles = Mass of substance / Molar mass

Number of moles = 9.0 grams / 18.0 grams/mole
Number of moles ≈ 0.50 moles

Now that we have the number of moles, we can calculate the heat evolved during the condensation:

Heat evolved = ΔH × Number of moles

Heat evolved = +44 kJ × 0.50 moles
Heat evolved = +22 kJ

Therefore, approximately 22 kJ of heat is evolved when 9.0 grams of water vapor is condensed to liquid water.

Reverse the equation to be H2O (g) --> H2O (l) delta H= -44kJ

There are 9.0 grams of H2O (g)
Find moles of the gas: 9.0/16= .50 moles
44 times .50 =22 kJ evolved