E
All the other chices give evidence that supports that hypothesisthat the Moon was made of material that was flung off Earth during a time when it was rapidly spinning.
Explanation:
There is an enormous amount of similarities between the minerals in the moon rocks and the rocks on earth, except that for some minerals, like potassium, their quantities are higher on the earth than on the moon.
However, there is still supports for the evidence (by the other choices) that the moon was made from a piece of earth ejected from asteroid impact in primordial earth.Explanation:It’s believed that more than 3.5 billion years during the formation of earth and before it had cooled there were frequent asteroid impacts and one enormous collision ejected a large piece of molten earth into space but within earth’s gravity influence. This piece formed the moon. Evidence of asteroid impacts are frozen in time on the moon surface thanks to the fact that the moon has no atmosphere or tectonic plates movements that wipe off this ‘evidence’.
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Answer: option <span>B.The total mass of A and C, which are carbon and oxygen, is equal to the mass of B, which is carbon dioxide.
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Explanation:
1) The combustion of carbon is represented by the chemical equation:
C + O₂ → CO₂
2) The law of conservation of mass states that the mass of the products is equal to the mass of the reactants.
3) The reactants are C and O₂, while the product is CO₂.
4) The masses given are: A: 12 g, B: 44 g, and C: 32 g
Then, 12g + 32 g = 44 g, this is A + C = B.
Then, B represents the product, which is CO₂, whose molar mass is 44 g/mol.
Since, the molar mass of C is 12 g/mol, it is A; and since the molar mass of O₂ is 32, it is C.
Therefore, the answer is the option B.
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Answer:
Explanation:
<u>1) Equilibrium equation (given)</u>:
- H₂ (g) + I₂ (g) ⇄ 2HI (g)
<u>2) Equilibrium constant expression</u>:
<u>3) Determine the conentrations from the stoichiometry</u>:
a) <u>Number of moles</u>:
H₂ (g) + I₂ (g) ⇄ 2HI (g)
Start 0.4 1.55 0
Change - 0.4×0.6 = - 0.24 - 0.24 + 0.24×2 = + 0.48
--------------------------- ------------- --------------------------
End 0.16 1.31 0.48
b) <u>Concentrations</u>:
- [ H₂ (g) ] = 0.16 mole / 2 liter = 0.08 M
- [ I₂ (g) ] = 1.31 mole / 2 liter = 0.655 M
- [HI (g) ] = 0.48 mole / 2 liter = 0.24 M
<u>4) Compute Kc</u>:
- Kc = (0.24 M)² / (0.08 M × 0.655 M) = 1.099 ≈ 1.1 ← answer
Answer:
Explanation:
2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O
The reaction above is a typical combustion reaction which are very common with hydrocarbons. Combustion occurs in the presence of oxygen to product carbon dioxide and water. The purpose of this reaction is to transform chemical energy into useful heat energy. Most times, the oxygen used is always in excess of the hydrocarbon reacting with it.