calculate the lowest frequency of UV. light which has enough energy to break a Cl-Cl bond. ( bond energy =243kj/mol). I got 7.89E14 but the answer is 6.14E14s–¹. how?
I saw the solution as ..E for 1 molecule is 243kj/mol / 6.022E23 molecules. I don't seem to understand that part.
To calculate the lowest frequency of UV light required to break a Cl-Cl bond, we need to use the equation that relates the energy of light to its frequency.
The equation is:
E = h * ν
Where:
E = energy of light (in joules)
h = Planck's constant (6.62607015 × 10^-34 J s)
ν = frequency of light (in Hz)
The bond energy of a Cl-Cl bond is given as 243 kJ/mol. To convert it to joules, we divide it by Avogadro's number:
243 kJ/mol / 6.022 × 10^23 molecules/mol ≈ 4.03 × 10^-19 J
Now, we can rearrange the equation to solve for the frequency:
ν = E / h
ν ≈ (4.03 × 10^-19 J) / (6.62607015 × 10^-34 J s) ≈ 6.09 × 10^14 Hz
Note that Hz is the unit for frequency, and it is equivalent to s^(-1). Therefore, the lowest frequency of UV light required to break the Cl-Cl bond is approximately 6.09 × 10^14 s^(-1) or 6.09 × 10^14 Hz.
The given answer of 6.14 × 10^14 s^(-1) could be slightly different due to rounding errors or the use of different values for physical constants.