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pshichka [43]
3 years ago
11

Describe how neutrons were discovered

Chemistry
1 answer:
xxMikexx [17]3 years ago
6 0
Originally scientists believed in the plum pudding model of the atom (sphere of positive charge surrounded by smaller spheres of negative charge) then Rutherford did his scattering experiment (he shot alpha particles at a piece of gold foil some particles passed straight through the empty space of the atom, some were slightly deflected as they were closer to the atom's nucleus and some were completely reflected because they were headed in the path of the atom's nucleus
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Classify the following as either Sexual or Asexual Reproduction. Explain your choice.
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A) Asexual
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3 years ago
For the following reaction, find the value of Q and predict the direction of change, given that a 1L flask initially contains 2
Tresset [83]

Answer:

C) Q < K, reaction will make more products

Explanation:

  • 1/8 S8(s)  + 3 F2(g)  ↔  SF6(g)

∴ Kc = 0.425 = [ SF6 ] / [ F2 ]³

∴ Q = [ SF6 ] / [ F2 ]³

∴ [ SF6 ] = 2 mol/L

∴ [ F2 ] = 2 mol/L

⇒ Q = ( 2 ) / ( 2³)

⇒ Q = 0.25

⇒ Q < K, reaction will make more products

 

5 0
3 years ago
7) The fuel used to power the booster rockets on the space shuttle is a mixture of aluminum metal and ammonium perchlorate. The
iren2701 [21]
TLDR: 6.53x10^5 g NH4ClO4

The stoichiometric coefficients (the numbers in front of the reactants and products) show that Aluminum and Ammonium Perchlorate are consumed at the exact same rate throughout the reaction: 3 parts of one to 3 parts of another.

1.5x10^5 grams of Aluminum, considering that the formula weight of Aluminum is 26.98 g/mol, is equal to 5,559.7 moles of Aluminum. This means that 5,559.7 moles of Ammonium Perchlorate are required to run the reaction to completion.

The formula weight of Ammonium Perchlorate is 117.49 grams a mole, and multiplying it by 5,559.7 moles to react to completion means that 6.53x10^5 grams of Ammonium Perchlorate is required for the reaction.
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In a second-order reaction (one that is second order in one reactant), cutting in half the concentration of that reactant will h
Keith_Richards [23]
rate 1 of the reaction = k [A]²

rate 2 of the reaction = k [A/2]² = k[A]² /4

We can see that rate of the reaction will be 4 times less.
8 0
4 years ago
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