For electromagnetic radiation with a wavelength of 576.3 nm:

(a) What is the frequency of the radiation (in s-1)? (b) What is the energy (in J) of one photon of
the radiation? (c) What is the energy (in kJ) of one mole of photons of the radiation
So a I go 5.202x10^14 b)3.447x10^-19. C im not sure how to do. I did my answer in b times avagadros constant divided by 1000j and got 207.6 kj. Am i right? An answer asap would really help

Also are a and b correct

wave equation: freq*wavelengt=speed light

a) freq=3E8/576.3E-9 correct
b) energy = Plancks constant* freq Not the way you did it.
c) onemoleengery=above enegy*avag number

To calculate the energy of one mole of photons, you can use the following steps:

(a) First, calculate the frequency of the radiation using the formula:

Frequency (ν) = Speed of light (c) / Wavelength (λ)

Given the wavelength of 576.3 nm, we need to convert it to meters (1 nm = 1 × 10^-9 m):

Wavelength (λ) = 576.3 nm = 576.3 × 10^-9 m

Using the speed of light value, c = 3 × 10^8 m/s:

Frequency (ν) = (3 × 10^8 m/s) / (576.3 × 10^-9 m)

Calculating this will give you the value for frequency in s^-1.

(b) To find the energy of one photon, you can use the equation:

Energy (E) = Planck's constant (h) * Frequency (ν)

Planck's constant (h) = 6.626 × 10^-34 J·s

Multiply this with the frequency calculated in part (a) to get the energy in joules (J).

(c) To find the energy of one mole of photons, you need to multiply the energy per photon from part (b) by Avogadro's number (N_A) and convert it to kilojoules (kJ) by dividing by 1000.

Avogadro's number (N_A) = 6.022 × 10^23 mol^-1

Multiply the value obtained in part (b) by Avogadro's number and divide by 1000 to get the energy in kilojoules (kJ).

Your answer for part (b) seems correct – 3.447 × 10^-19 J per photon.

For part (c), the calculation would be:

Energy of one mole of photons = (3.447 × 10^-19 J/photon) * (6.022 × 10^23 mol^-1) / 1000

Evaluating this calculation will give you the energy in kilojoules (kJ) per mole of photons.

Please perform the calculations to find the exact value for part (c) and let me know if you have any further questions!

To calculate the energy of one mole of photons of the given electromagnetic radiation, we need to use the Avogadro's constant (6.022 x 10^23) to convert the quantity from one photon to mol.

(a) To determine the frequency of the radiation (in s^-1), we can use the formula:

frequency = speed of light / wavelength

Given that the wavelength is 576.3 nm (or 576.3 x 10^-9 meters) and the speed of light is approximately 3 x 10^8 meters per second:

frequency = (3 x 10^8 m/s) / (576.3 x 10^-9 m)
frequency ≈ 5.203 x 10^14 s^-1

Therefore, your calculated frequency of 5.202 x 10^14 s^-1 is correct.

(b) To determine the energy (in J) of one photon, we can use the equation:

energy = Planck's constant x frequency

The Planck's constant is approximately 6.626 x 10^-34 J·s:

energy = (6.626 x 10^-34 J·s) x (5.203 x 10^14 s^-1)
energy ≈ 3.448 x 10^-19 J

Hence, your calculated energy for one photon, 3.447 x 10^-19 J, is correct.

(c) To calculate the energy of one mole of photons, we can multiply the energy of one photon (in J) by the Avogadro's constant and convert it to kJ:

energy of one mole of photons = (energy of one photon x Avogadro's constant) / 1000

energy of one mole of photons = (3.447 x 10^-19 J) x (6.022 x 10^23 photons/mol) / 1000
energy of one mole of photons ≈ 207.6 kJ

Therefore, your calculated energy of one mole of photons as 207.6 kJ is correct.

Keep in mind that the answers have been rounded for simplicity.