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34kurt
2 years ago
13

What is the energy of a 933 nm wave?

Chemistry
2 answers:
vovikov84 [41]2 years ago
8 0

E=hc/l

E=

<span><span>E=<span>(6.626 x 10-34 J s)(3.0 x 108m/s )</span><span>=2.88 x 10-19J</span></span><span>6.90 x 10-7m</span></span>
Natali [406]2 years ago
4 0

Answer: 0.02130\times 10^{-17}Joules

Explanation:

E=\frac{hc}{\lambda}

E= energy

h = Planck's constant = 6.626\times 10^{-34}Js

c = speed of light =3\times 10^8ms^{-1}

\lambda = Wavelength of radiation = 933 nm =933\times 10^{-9}m

Now put all the given values in this formula, we get

E=\frac{6.626\times 10^{-34}Js\times 3\times 10^8ms^{-1}}{933\times 10^{-9}m}

E=0.02130\times 10^{-17}Joules

Thus energy of a 933 nm wave is 0.02130\times 10^{-17}Joules

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Answer:

The best practices officers should use when securing a crime scene is option D

D. They should secure a larger area than the actual crime scene

Explanation:

Officers should secure the scene by limiting access to the scene and movement within the scene

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2 years ago
I NEED HELP PLEASE!!!! CHEMISTRY QUESTION: If 38 g of Li3P and 15 grams of Al2O3 are reacted, what total mass of products will r
maksim [4K]

Answer:

21.5 g.

Explanation:

Hello!

In this case, since the reaction between the given compounds is:

2Li_3P+Al_2O_3\rightarrow 3Li_2O+2AlP

We can see that according to the law of conservation of mass, which states that matter is neither created nor destroyed during a chemical reaction, the total mass of products equals the total mass of reactants based on the stoichiometric proportions; in such a way, we first need to compute the reacted moles of Li3P as shown below:

n_{Li_3P}^{reacted}=38gLi_3P*\frac{1molLi_3P}{51.8gLi_3P}=0.73molLi_3P

Now, the moles of Li3P consumed by 15 g of Al2O3:

n_{Li_3P}^{consumed \ by \ Al_2O_3}=15gAl_2O_3*\frac{1molAl_2O_3}{101.96gAl_2O_3} *\frac{2molLi_3P}{1molAl_2O_3} =0.29molLi_3P

Thus, we infer that just 0.29 moles of 0.73 react to form products; which means that the mass of formed products is:

m_{Li_2O}=0.29molLi_3P*\frac{3molLi_2O}{2molLi_3P} *\frac{29.88gLi_2O}{1molLi_2O} =13gLi_2O\\\\m_{AlP}=0.29molLi_3P*\frac{2molAlP}{2molLi_3P} *\frac{57.95gAlP}{1molAlP} =8.5gAlP

Therefore, the total mass of products is:

m_{products}=13g+8.5g\\\\m_{products}=21.5g

Which is not the same to the reactants (53 g) because there is an excess of Li₃P.

Best Regards!

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