The energy required to break one mole of Cl-C | vedclass

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(D) Energy required to break one mole of $Cl_2$ molecules is $242 \, kJ \, mol^{-1} = 242 	imes 10^3 \, J \, mol^{-1}.$Energy required to break a sin

Vedclass · Accepted Answer

$494$

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(D) Energy required to break one mole of $Cl_2$ molecules is $242 \, kJ \, mol^{-1} = 242 	imes 10^3 \, J \, mol^{-1}.$Energy required to break a single $Cl-Cl$ bond is $E = \frac{242 	imes 10^3}{6.02 	imes 10^{23}} \, J.$Using the relation $E = \frac{hc}{\lambda}$,the wavelength is $\lambda = \frac{hc}{E}.$Substituting the values: $\lambda = \frac{6.626 	imes 10^{-34} \, J \cdot s 	imes 3 	imes 10^8 \, m \cdot s^{-1} 	imes 6.02 	imes 10^{23} \, mol^{-1}}{242 	imes 10^3 \, J \cdot mol^{-1}}.$$\lambda \approx 4.94 	imes 10^{-7} \, m = 494 	imes 10^{-9} \, m = 494 \, nm.$

The energy required to break one mole of $Cl-Cl$ bonds in $Cl_2$ is $242 \, kJ \, mol^{-1}.$ The longest wavelength of light capable of breaking a single $Cl-Cl$ bond is $............ \, nm.$
$(c = 3 \times 10^8 \, m \, s^{-1}$ and $N_A = 6.02 \times 10^{23} \, mol^{-1}).$

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The energy required to break one mole of $Cl-Cl$ bonds in $Cl_2$ is $242 \, kJ \, mol^{-1}.$ The longest wavelength of light capable of breaking a single $Cl-Cl$ bond is $............ \, nm.$$(c = 3 \times 10^8 \, m \, s^{-1}$ and $N_A = 6.02 \times 10^{23} \, mol^{-1}).$