the energy required to break one mole of chlorine- chlorine bonds in Cl2 is 242 kj/mol. what is the longest wavelength of light capable of breaking a single Cl-Cl bond?
242 kJ/mol. Convert t J and divide by 6.022E23 to convert to 1 molecule. Then
E = hc/wavelength
Thank you I got 494 nm
I may may have punched in a wrong number on my calculator but I obtained 494.65 nm which would round to 495 nm.
To find the longest wavelength of light capable of breaking a single Cl-Cl bond, we need to consider the energy required to break the bond and relate it to the wavelength using the equation E = hc/λ.
First, we need to convert the given energy from kilojoules (kJ) to joules (J) since the SI unit of energy is Joules.
1 kJ = 1000 J
Therefore, 242 kJ/mol = 242,000 J/mol
Next, we need to convert the energy per mole of Cl-Cl bonds to the energy required to break a single Cl-Cl bond by dividing it by Avogadro's number (6.022 × 10^23/mol).
Energy per bond = 242,000 J/mol / (6.022 × 10^23/mol) = 4.02 × 10^(-19) J/bond
Now we can use the equation E = hc/λ to find the corresponding wavelength.
Where:
E = energy of the photon (in Joules)
h = Planck's constant (6.626 × 10^(-34) J·s)
c = speed of light (2.998 × 10^8 m/s)
λ = wavelength of light (in meters)
Rearranging the equation, we have λ = hc/E
Plugging in the given values, we get:
λ = (6.626 × 10^(-34) J·s × 2.998 × 10^8 m/s) / (4.02 × 10^(-19) J)
Calculating the expression, we find:
λ ≈ 4.94 × 10^(-7) meters
Therefore, the longest wavelength of light capable of breaking a single Cl-Cl bond is approximately 4.94 × 10^(-7) meters or 494 nanometers (nm).