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AURORKA [14]
3 years ago
10

How was Earth’s atmosphere changed during the Great Oxygenation Event?

Chemistry
2 answers:
SpyIntel [72]3 years ago
8 0

Consequences of oxygenation. Eventually, oxygen started to accumulate in the atmosphere, with two major consequences. Oxygen likely oxidized atmospheric methane (a strong greenhouse gas) to carbon dioxide (a weaker one) and water.

faust18 [17]3 years ago
3 0

Answer: .Early organisms created oxygen from other gases in the atmosphere

Explanation:

It is believed that the atmosphere emerged about 4,500 million years ago, by a process that can be explained in five stages.

In the first stage, the atmosphere was shaped by volcanic emanations, such as water vapor, carbon and sulfur dioxide, and nitrogen. At this point, oxygen was barely present.

In the second stage, as the Earth cooled, the water vapor condensed and formed the oceans. Carbon dioxide reacted with the rocks of the earth's crust to create carbonates - (CO32-); a portion of them, when dissolved in the seas, generated salt water.

In the third stage, approximately 3.500 million years ago, bacteria appear, capable of carrying out photosynthesis, that is, of producing oxygen. This facilitated the development of marine life.

Once the atmosphere obtained sufficient oxygen, the fourth stage appeared, the evolution of large organisms as animals capable of breathing air.

This is how the current atmosphere containing the gases created in each of the previous phases was reached. These are kept in motion by winds and rains, allowing humans, and other living organisms, to breathe. For this reason, without them there would be no life on the planet.

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How many number of atoms does these have?
Olin [163]

Answer:

Explanation:

16. 12

17. 8

18. 9

19. 10

20. 5

21. 15

22.8

23. 24

24. 12

25. 3 i guess( some one comment for 25th pls)

26. 2

3 0
3 years ago
2. Calculate the mass of solvent in grams in a solution containing 3.0 grams of Tylenol
katrin2010 [14]

Answer:

  • <u>83g</u>

Explanation:

<u>1, Formula</u>

  • Mass percent = (mass of solute/mass of solution) × 100

<u>2. Determine mass of solution</u>

Substitute the data and clear the mass of solution:

  • 3.5 = (3.0g / mass of solution) × 100
  • 0.035 = 3.0g / mass of solution
  • mass of solution = 3.0 g / 0.035
  • mass of solution = 85.714g

<u>3. Determine the mass of solvent:</u>

  • mass of solvent = mass of solution - mass of solute
  • mass of solvent = 85.714g - 3.0g = 82.714g

Round to two significant figures: 83 g

3 0
3 years ago
4. A 0.100 M solution of NaOH is used to titrate an HCl solution of unknown concentration. To neutralize the solution, an averag
PtichkaEL [24]

Answer:

C. 0.191 M

Explanation:

Our goal for this question, is to calculate the concentration of the HCl solution. For this, in the experiment, a solution of NaOH was used to find the moles of HCl. Therefore, our first step is to know the <u>reaction between HCl and NaOH</u>:

HCl~+~NaOH~->~NaCl~+~H_2O

The "<u>titrant"</u> in this case is the NaOH solution. If we know the concentration of NaOH (0.100M) and the volume of NaOH (38.2 mL=0.0382 L), we can calculate the moles using the <u>molarity equation</u>:

M=\frac{mol}{L}

0.100~M=\frac{mol}{0.0382~L}

mol=0.100~M*0.0382~L=0.0382~mol~of~NaOH

Now, in the reaction, we have a <u>1:1 molar ratio</u> between HCl and NaOH (1 mol of HCl is consumed for each mole of NaOH added). Therefore we will have the same amount of moles of HCl in the solution:

0.0382~mol~of~NaOH\frac{1~mol~HCl}{1~mol~NaOH}=0.0382~mol~HCl

If we want to calculate the molarity of the HCl solution we have to <u>divide by the litters</u> of HCl used in the experiment (20 mL= 0.02 L):

\frac{0.0382~mol~HCl}{0.02~L}~=~0.191~M

The concentration of the HCl solution is 0.191 M

I hope it helps!

8 0
3 years ago
How many moles of ammonia are produced by 5 moles of hydrogen.
hichkok12 [17]

Answer: 10 moles

Explanation:

8 0
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A chemical formula is shown below. How many total atoms are in 2 molecules of the chemical formula shown?
Lilit [14]

Answer: 42

Explanation: I took a quiz and had the same question.

6 0
4 years ago
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