   Chapter 23, Problem 3PS

Chapter
Section
Textbook Problem

Is violet light (with a wavelength of 400 nm) sufficiently energetic to break a carbon-carbon single bond (the average C-C bond energy is 346 kJ/mol)?

Interpretation Introduction

Interpretation: The violet light is whether sufficent to break the carbon-carbon single bond or not has to be determined.

Concept introduction:

All the saturated hydrocarbons have carbon-carbon single bonds. The energy required to break a carbon-carbon bond is 346 kJ/mol. This much amount of energy can be provided by extreme hight or via a sunlight at lower wavelenght.

When violet light is applied the wavelength is 400 nm. The enegy provided by this wavelength is calculated by using following expression,

E=hcλ

Here, h is the Planck’s constant, c is the speed of light and λ is the wavelength of light.

Explanation

The calculation of energy is given below.

Given:

The value of wavelenght (λ) for violet light is 400 nm or 400×109m.

Value of Planck’s constant (h) is 6.626×1034Js.

Speed of light is equals to 3×108ms1.

Enegry is calculated by using equation (1).

E=hcλ

Substitute the values,

E=(6.626×1034Js)(3×108ms1)(400×109m)=4

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