A photon having $λ = 800 A$ causes the ionization of a nitrogen atom. The $I . E .$ per mole of nitrogen in $K J$ is?
$[G i v e n : E = 1240 e V - n m, 1 e V = 96.43 K J / m o l]$

1495.42 K J / m o l

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1500.56 K J / m o l

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1634.87 K J / m o l

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1567.32 K J / m o l

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Solution

The correct option is A $1495.42 K J / m o l$
The energy of one photon of wavelength 800 A is:

$E = \frac{h c}{λ} = \frac{6.6256 \times 10^{- 34} J s \times 2.9979 \times 10^{8} m / s}{800 \times 10^{- 10} m}$

$= 2.476 \times 10^{- 18} J = 2.47 \times 10^{- 21} k J$

The energy for one mole of photons is:

$E = 6.023 \times 10^{23} \times 2.476 \times 10^{- 21} k J$

$= 1495.42 k J / m o l .$

Hence, the correct option is $A$

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Similar questions

An electromagnetic radiation of wavelength 242 nm is just sufficient to ionize a sodium atom. Calculate the ionization energy of sodium in kJ ${m o l}^{- 1}$ .

Q. Atoms can form a variety of bonds with other atoms. Example of bonding types include ionic, covalent, and metallic.

Element	$1^{s t} I . E .$	$2^{n d} I . E .$	$3^{r d} I . E .$	Electronegativity
$A l$	$580 k J / m o l$	$1820 k J / m o l$	$2740 k J / m o l$	$1.5$
$C$	$1100 k J / m o l$	N/A	N/A	$2.5$
$H$	$1310 k J / m o l$	N/A	N/A	$2.1$
$B$	$800 k J / m o l$	N/A	N/A	$2.0$
$F$	$1680 k J / m o l$	N/A	N/A	$4.0$
$M g$	$735 k J / m o l$	$1450 k J / m o l$	N/A	$1.2$