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tester [92]
2 years ago
7

Is there more than one possible model that could be inferred from Rutherford’s data?

Chemistry
2 answers:
tankabanditka [31]2 years ago
8 0

Answer:

your missing the rest?

Explanation:

i dont know

AlexFokin [52]2 years ago
7 0
Rutherford's model of atoms represented the solar system. Where the positive charge is at the centre like the sun and electrons revolve around it like a planet. Therefore, his model is known as planetary model.
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What is the energy in joules of one photon of<br> microwaveradiation with a wavelength 0.122m?
pentagon [3]

<u>Answer:</u> The energy of photon is 162.93\times 10^{-26}J

<u>Explanation:</u>

The relation between energy and wavelength of light is given by Planck's equation, which is:

E=\frac{hc}{\lambda}

where,

E = energy of the light  = ?

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

c = speed of light = 3\times 10^8m/s

\lambda = wavelength of photon = 0.122 m

Putting values in above equation, we get:

E=\frac{(6.626\times 10^{-34}Js)\times (3\times 10^8m/s)}{0.122m}\\\\E=162.93\times 10^{-26}J

Hence, the energy of photon is 162.93\times 10^{-26}J

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3 years ago
What are some of the body external defenses
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There are 7 named classes of hazardous materials.<br> O True<br> O False
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7 0
2 years ago
1.12g H2 is allowed to react with 9.60 g N2, producing 1.23 g NH3.
andriy [413]

Answer:

A. m_{NH_3}^{theo} =1.50gNH_3

B. Y=82.2\%

Explanation:

Hello!

In this case, since the undergoing chemical reaction between nitrogen and hydrogen is:

N_2+3H_2\rightarrow 2NH_3

Thus we proceed as follows:

A. Here, we first need to compute the moles of ammonia yielded by each reactant, in order to identify the limiting one:

n_{NH_3}^{by \ H_2}=1.12gH_2*\frac{1molH_2}{2.02gH_2}*\frac{2molNH_3}{3molH_2}=0.370molNH_3\\\\  n_{NH_3}^{by \ N_2}=1.23gN_2*\frac{1molN_2}{28.02gN_2}*\frac{2molNH_3}{1molN_2}=0.0878molNH_3

Thus, since nitrogen yields the fewest moles of ammonia, we realize it is the limiting reactant, so the theoretical yield, in grams, of ammonia is:

m_{NH_3}^{theo}=0.0878mol*\frac{17.04gNH_3}{1molNH_3} =1.50gNH_3

B. Finally, since the actual yield of ammonia is 1.23, the percent yield turns out:

Y=\frac{1.23gNH_3}{1.50gNH_3} *100\%\\\\Y=82.2\%

Best regards!

5 0
3 years ago
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