The enthalpy of vaporization at 298 K for diethylether (C4H10C) is 26.0 kj/mol. How much heat would be required to vaporize 1.00 L of the ether at 298 K if its density is 0.714 g/L ?

A) 250 kj
B) 74.1 kj
C) 186 kj
D) 130 kj
E) 440 kj

Well, well, well, we have an enthalpy question here! Let's tackle it with a dash of humor.

To begin with, we need to find the number of moles of diethyl ether. Since the density is given as 0.714 g/L and we have 1.00 L of ether, we can calculate the mass of the ether using the density and volume.

1.00 L * 0.714 g/L = 0.714 g

Now we need to convert the mass to moles using the molar mass of diethyl ether (74.12 g/mol).

0.714 g / 74.12 g/mol ≈ 0.00963 mol

Now that we have the number of moles, we can use the enthalpy of vaporization (26.0 kJ/mol) to calculate the heat required.

Heat = Enthalpy of vaporization * Number of moles
Heat = 26.0 kJ/mol * 0.00963 mol ≈ 0.250 kJ

So the heat required to vaporize 1.00 L of diethyl ether at 298 K is approximately 0.250 kJ.

Now, let's find the option that matches our answer. Drumroll, please!

Hmm, option A) 250 kJ seems to be the closest in value. But hold your horses! They seem to have mixed up the units. They gave the answer in kJ, while we found our answer in kJ/mol. Silly, silly!

Seems like someone needs a lesson in units. So, the correct answer is not A) 250 kJ, but in fact, it's B) 74.1 kJ! That's right folks, option B) is the winner! Ta-dah!

Remember, chemistry can be quite a circus sometimes, but with a little humor, we can make it fun!

To calculate the heat required to vaporize 1.00 L of diethylether (C4H10C), we need to use the formula:

Heat = Enthalpy of Vaporization × Amount of Substance

Step 1: Convert the density to the amount of substance (moles)
Since we're given the density of ether (0.714 g/L), we can calculate the amount of substance (moles) using the molar mass of diethylether (74.12 g/mol).

Amount of Substance = Density × Volume / Molar Mass
Amount of Substance = (0.714 g/L) × (1.00 L) / (74.12 g/mol)

Step 2: Calculate the heat required
Heat = Enthalpy of Vaporization × Amount of Substance
Heat = (26.0 kJ/mol) × (Amount of Substance)

Step 3: Perform the calculation
Substitute the value of Amount of Substance into the equation:

Heat = (26.0 kJ/mol) × ((0.714 g/L) × (1.00 L) / (74.12 g/mol))

Heat = 0.260 kJ

Therefore, the amount of heat required to vaporize 1.00 L of diethylether is 0.260 kJ.

Since none of the provided options match the calculated answer, it seems that there might be a mistake in the answer choices.

To determine the heat required to vaporize 1.00 L of diethylether (C4H10O) at 298 K, you need to make use of the formula:

Heat = enthalpy of vaporization × moles of substance

The given density of diethylether is 0.714 g/L. To find the moles of diethylether in 1.00 L, you must convert the density to moles using its molar mass.

The molar mass of diethylether (C4H10O) is:

(4 × molar mass of carbon) + (10 × molar mass of hydrogen) + (1 × molar mass of oxygen) = (4 × 12.01 g/mol) + (10 × 1.01 g/mol) + (1 × 16.00 g/mol)

= 60.10 g/mol

Now, to calculate the moles, divide the given mass by the molar mass:

moles = mass / molar mass

moles = (0.714 g/L) / (60.10 g/mol)

moles = 0.0119 mol/L

Since we want to find the heat required to vaporize 1.00 L of the ether, we can multiply the moles by 1.00 L:

moles = 0.0119 mol/L × 1.00 L = 0.0119 mol

Now, substitute the values into the formula:

Heat = (26.0 kJ/mol) × (0.0119 mol)

Heat = 0.3094 kJ

To convert kJ to J, multiply by 1000:

Heat = 0.3094 kJ × 1000 = 309.4 J

Now, to convert J to kJ, divide by 1000:

Heat = 309.4 J / 1000 = 0.3094 kJ

Therefore, the heat required to vaporize 1.00 L of diethylether at 298 K is approximately 0.3094 kJ. However, none of the answer choices matches this value exactly. It seems there may be a mistake in the options provided or in the calculations.

q = mass x heat vap

You can get the mass from the density and volume.