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3 years ago

How much energy does a 930 nm wave of light have? (The speed of light in a

Chemistry

1 answer:

Orlov [11]3 years ago

4 0

Answer:

$E=2.14\times 10^{-19}\ J$

Explanation:

We have,

Wavelength of a light is 930 nm

It is required to find the energy of a wave of light. The energy of a wave is given in terms of following as :

$E=\dfrac{hc}{\lambda}\\\\E=\dfrac{6.626\times 10^{-34}\times 3\times 10^8}{930\times 10^{-9}}\\\\E=2.14\times 10^{-19}\ J$

So, the energy of the wave is $2.14\times 10^{-19}\ J$

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Answer:

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3 years ago

Balance <br><br> _Mg + _HCL = _MgCl2 + H2

Pavel [41]

_Mg + _HCL = _MgCl2 + H2
Separate the terms on each side:

_Mg + _HCl = _MgCl2 + H2

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1Mg

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2HCl

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3 years ago

Read 2 more answers

How many atoms are in 68.44 grams

creativ13 [48]

Correct answer There are 68 grams are in atoms

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3 years ago

The expected o-c-h angle in this molecule is degrees. the expected hybridization at the central carbon is

WINSTONCH [101]

Each neutral carbon atom contains four valence electrons and may form up to four electron domains. Possible hybridizations include

$sp^{3}$ , four electron domains, as in ethane $\text{C}_2\text{H}_6$
$sp^{2}$ , three electron domains, as in ethene $\text{C}_2\text{H}_4$
$sp$ , two electron domains, as in ethyne $\text{C}_2\text{H}_2$

Molecules of each of the three hybridization demonstrate spatial configurations that would maximizes the separation between the electron domains.

Carbon atoms with a $sp^{3}$ hybridization would demonstrate a tetrahedral configuration with a bond angle of approximately $109.5\textdegree{}$
Carbon atoms with a $sp^{2}$ hybridization would demonstrate a triangular planar configuration with a bond angle of $120\textdegree{}$
Carbon atoms with a $sp$ hybridization would demonstrate a linear configuration with a bond angle of $180\textdegree{}$

Bond angles are characteristic of the spatial configuration of electron domains and identifies the hybridization of the central carbon atom.

Note that each hydrogen atom contains only one valence electron and would form only single bonds. It takes two valence electrons for oxygen atoms to achieve an octet such that each oxygen form only two bonds at a single time. Therefore given the fact that the carbon is bonded to both hydrogen and oxygen, only the following hybridizations are possible

$sp^{3}$ in which the oxygen atom forms a carbon-oxygen double bond with the central carbon atom;
$sp^{2}$ in which the oxygen atom forms a single bond with the central carbon atom and with a second atom.

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4 years ago