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Fofino [41]
3 years ago
6

8. Sulfur has a first ionization energy of 1000 kJ/mol. Photons of what frequency are required to ionize one mole of Sulfur?​

Chemistry
1 answer:
Lynna [10]3 years ago
6 0

Answer:

the frequency of photons v = 1.509\times10^{39}Hz

Explanation:

Given:  first ionization energy of 1000 kJ/mol.

No. of moles of sulfur = 1 mole

\Delta E_1 = 1000KJ/mol

We know that plank's constant

h = 6.626\times10^{-34} Js

Let the frequency of photons be ν

Also we know that ΔE = hν

this implies ν = ΔE/h

= \frac{10^6J}{6.626\times10^{-34} Js}

v = 1.509\times10^{39}Hz

Hence, the frequency of photons v = 1.509\times10^{39}Hz

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Mass of Li = 237.38 g

<h3>Further explanation</h3>

The mole itself is the number of particles contained in a substance amounting to 6.02.10²³  

\large {\boxed {\boxed {\bold {mol = \frac {mass} {molar \: mass}}}}

<h3>Known</h3>

Moles of Li = 34.2

Molar mass(MW) of Li = 6.941 g/mol

then mass of Lithium (Li) :

\tt mol=\dfrac{mass}{MW}\\\\mass=mol\times MW\\\\mass=34.2\times 6,941~g/mol\\\\mass=\boxed{\bold{237.38~g}}

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