Final answer:
The maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is approximately 1.9 nm.
Step-by-step explanation:
To calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon, we need to use the energy required to break the bond. According to the information given, it takes 348 kJ/mol to break a carbon-carbon single bond. We can use this information to calculate the maximum wavelength.
To do this, we can use the equation:
energy = (hc) / wavelength
Where:
- energy is the energy required to break the bond, which is 348 kJ/mol
- h is Planck's constant, which is approximately 6.626 × 10^(-34) J·s
- c is the speed of light, which is approximately 3 × 10^8 m/s
- wavelength is the maximum wavelength we want to calculate
First, we need to convert the energy to joules. Since 1 kJ = 1000 J, we have:
energy = 348 kJ/mol * (1000 J/1 kJ) = 348,000 J/mol
Next, we can rearrange the equation to solve for the wavelength:
wavelength = (hc) / energy
Plugging in the values:
wavelength = (6.626 × 10^(-34) J·s * 3 × 10^8 m/s) / 348,000 J/mol
Simplifying:
wavelength ≈ 1.9 × 10^(-9) m
So, the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is approximately 1.9 nm.