Calculate the heat in kilojoules needed to condense 185g of steam at 100 ∘C.

Well, I may be a funny bot, but I do know a thing or two about heat! To calculate the heat needed to condense 185g of steam at 100 ∘C, we need to consider the heat of vaporization of water.

The heat of vaporization for water is approximately 40.7 kJ/mol. Since you've given me the mass (185g) and not the number of moles, we first need to convert the mass of steam to moles.

The molar mass of water is 18.015 g/mol. So, we can calculate the number of moles using the following equation:
moles = mass / molar mass
moles = 185g / 18.015 g/mol

Once we have the number of moles of water, we can calculate the heat using the equation:
heat = moles x heat of vaporization

Now, let me get my calculator...
*Clown Bot pulls out a ridiculously large calculator*

185g / 18.015 g/mol = approximately 10.27 moles

heat = 10.27 moles x 40.7 kJ/mol = approximately 418.7 kJ

So, approximately 418.7 kilojoules of heat are needed to condense 185g of steam at 100 ∘C.

To calculate the heat required to condense 185g of steam at 100°C, we need to consider two main steps:

Step 1: Calculate the heat required to cool the steam from 100°C to 100°C (latent heat)
Step 2: Calculate the heat required to condense the steam at 100°C (latent heat of vaporization)

Step 1: Calculating the heat required to cool the steam from 100°C to 100°C
The specific heat capacity of steam is approximately 2.03 J/g°C.
To calculate the heat required to cool the steam, we use the formula:

Heat = mass × specific heat capacity × temperature change

In this case, the temperature change is from 100°C to 100°C, which is 0°C. Therefore, the heat required in this step is:

Heat = 185g × 2.03 J/g°C × 0°C = 0 J

Step 2: Calculating the heat required to condense the steam at 100°C
The latent heat of vaporization, L, for water is approximately 2260 J/g.

To calculate the heat required to condense the steam, we use the formula:

Heat = mass × latent heat of vaporization

Using the given mass of 185g, we can calculate the heat in this step:

Heat = 185g × 2260 J/g = 418,100 J

Finally, to convert the heat from joules to kilojoules, we divide by 1000:

Heat in kilojoules = 418,100 J / 1000 = 418.1 kJ

Therefore, the heat required to condense 185g of steam at 100°C is 418.1 kJ.

To calculate the heat needed to condense a substance, we need to know its specific heat capacity (C) and the change in temperature (ΔT).

In this case, we are dealing with steam at 100°C condensing into liquid water at 100°C. At this temperature, the steam undergoes a phase change from gas to liquid. The heat required for this phase change is called the latent heat of vaporization (Lv).

First, let's calculate the heat required to raise the temperature of 185g of steam from 100°C to 100°C:

Q1 = m * C * ΔT

Where:
Q1 is the heat needed
m is the mass of the substance (185g)
C is the specific heat capacity of water (4.184 J/g°C)
ΔT is the change in temperature (100 - 100 = 0°C)

Q1 = 185g * 4.184 J/g°C * 0°C
Q1 = 0 J

Since there is no change in temperature during the phase change, the heat required for this step is zero.

Next, let's calculate the heat required for the phase change from gas to liquid:

Q2 = m * Lv

Where:
Q2 is the heat needed
m is the mass of the substance (185g)
Lv is the latent heat of vaporization for water (2260 J/g)

Q2 = 185g * 2260 J/g
Q2 = 417,100 J

Finally, let's convert the heat from joules to kilojoules:

Q2 = 417,100 J / 1000
Q2 = 417.1 kJ

Therefore, the heat needed to condense 185g of steam at 100°C is 417.1 kilojoules (kJ).

To do this, you need the the latent heat of vaporization (Lv) for water.

In references, the Lv for water is 2256 J/g.
The formula for the heat released of absorbed is
Q = m * Lv
where
m = mass
Lv = heat of vaporization
In this case, heat is released (negative Q) because the steam is condensed.
Substituting,
Q = 185 * 2256
Q = ?

Now solve for Q. Units are in J so divide it by 1000 to convert it to kJ.

Hope this helps :3