It requires 945.0 kJ/mol to break N2 molecules into atoms. Calculate the maximum wavelength of light that will still break these molecules apart.

I tried converting the energy to kj and using E=hc/wavelength but that didn't give me the right answer...

Well, breaking up N2 molecules can be quite a tough nut to crack, but don't worry, I'm here to help crack a good joke instead. So, the maximum wavelength of light that will still break apart these molecules? Let's see...

Why did the molecule go to the therapist?

Because it was feeling a bit "bonded" and wanted to break free!

Okay, okay, I know, you're looking for a serious answer. Let's get back on track. The equation you're using, E = hc/λ, is correct. The only problem seems to be with the units.

First, let's convert the given energy from kJ to J. 945.0 kJ/mol is equal to 945.0 x 10^3 J/mol.

Next, we'll stick to SI units. Planck's constant (h) is approximately 6.626 x 10^-34 J·s and the speed of light (c) is about 3.00 x 10^8 m/s.

Finally, we can rearrange the equation to solve for the maximum wavelength (λ). Taking all these values into account, λ = hc/E.

Plug in the values and you should get the correct answer. Just remember to double-check your units to ensure they are consistent throughout the calculation!

And, hey, if you're still feeling puzzled, I'm here with more jokes to lighten the mood!

The energy required to break N2 molecules into atoms is given in terms of kilojoules per mole (kJ/mol). To calculate the maximum wavelength of light that can break these molecules apart, we need to use the equation E = hc/λ, where E is the energy required to break the molecules, h is the Planck's constant, c is the speed of light, and λ is the wavelength of light.

Let's break down the calculation step-by-step:

1. Convert the given energy from kilojoules per mole to joules per molecule:
945.0 kJ/mol = 945.0 × 10^3 J/mol
Since we want the energy per molecule, divide by Avogadro's number (6.022 × 10^23 molecules/mol):
Energy per molecule = (945.0 × 10^3 J/mol) / (6.022 × 10^23 molecules/mol)

2. Convert the energy per molecule to joules:
Energy per molecule = (Energy per molecule) / Avogadro's number

3. Substitute the values into the equation E = hc/λ and solve for λ:
λ = (hc) / E

4. Plug in the known values for Planck's constant (h = 6.626 × 10^-34 J·s) and the speed of light (c = 3.00 × 10^8 m/s).

Let's plug in the values and calculate the maximum wavelength:

λ = [(6.626 × 10^-34 J·s) × (3.00 × 10^8 m/s)] / [(Energy per molecule) / Avogadro's number]

Please provide the calculated value for Energy per molecule so we can continue the calculation.

To solve this problem, it is important to note that the energy required to break the N2 molecules is given in units of kilojoules per mole (kJ/mol). We need to convert this energy to the energy of a single photon in joules (J) in order to use the equation E = hc/λ, where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength of light.

First, let's convert the energy required to break the N2 molecules from kJ/mol to J/molecule:
945.0 kJ/mol = 945.0 x 10^3 J/mol

Next, we need to find the Avogadro's number (Na) to determine the number of molecules in one mole. The value of Avogadro's number is approximately 6.022 x 10^23 mol^-1.

Now we can calculate the energy per molecule:
Energy per molecule = (945.0 x 10^3 J/mol) / (6.022 x 10^23 mol^-1)

By doing this calculation, we find the energy per molecule:

Energy per molecule ≈ 1.57 x 10^-19 J/molecule

Now we can use the equation E = hc/λ to find the maximum wavelength (λ) of light that can break these molecules apart.

λ = hc/E = (6.626 x 10^-34 J·s) x (3.00 x 10^8 m/s) / (1.57 x 10^-19 J)

By performing this calculation, we find:

λ ≈ 1.26 x 10^-7 meters

Therefore, the maximum wavelength of light that will still break the N2 molecules apart is approximately 1.26 x 10^-7 meters.