Question

It takes 839./kJmol to break a carbon-carbon triple bond. Calculate the maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon.

Round your answer to 3 significant digits in nm.

Answer 1

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.

Step-by-step explanation:

It takes 839 kJ/mol to break a carbon-carbon triple bond.

Energy required to break 1 mole of carbon-carbon triple bond = E = 839 kJ

E = 839 kJ/mol = 839,000 J/mol

Energy required to break 1 carbon-carbon triple bond = E'

`E'=( 839,000 J/mol)/(N_A)=(839,000 J)/(6.022* 10^(23) mol^(-1))=1.393* 10^(-18) J`

The energy require to single carbon-carbon triple bond will corresponds to wavelength which is required to break the bond.

`E'=(hc)/(\lambda )` (Using planks equation)

`\lambda =(6.626* 10^(-34) Js* 3* 10^8 m/s)/(1.393* 10^(-18) J)`

`\lambda =1.427* 10^(-7) m =142.7 nm = 143 nm`

`(1 m = 10^9 nm)`

The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.