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Murrr4er [49]
4 years ago
14

Please give a brief explanation on all the types of clouds, like stratus, Stratocumulus and etc

Chemistry
1 answer:
blondinia [14]4 years ago
8 0
When water on land or in the ocean evaporates - turns from a liquid to water vapor - it rises. The water vapor cools and turns back into a liquid in the shape of tiny droplets. The result is clouds, unless it's on the ground - then we call it fog. When enough droplets get together they fall to the ground as rain or if it's very cold, they freeze and fall down as snow, sleet or hail. Clouds play an important role in the energy balance of Earth. They cool the earth by reflecting sunlight back out to space. How else do you think astronauts see where they are going? More importantly, clouds replenish our water supply. It's a never-ending cycle but one that keeps the earth balanced. You can tell a lot by looking at a cloud's shape, size and texture. Clouds are put into categories according to their shape, how high they are in the sky, their size, how fast and in what direction they are moving, etc. The three different types of clouds are high clouds (because they are high in the sky), medium clouds and low clouds (just over 10,000 feet high or 3 km.)
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How many grams of sulfuric acid is needed to neutralize 380 ml of solution with pH = 8.94
erma4kov [3.2K]

Answer : The mass of sulfuric acid needed is 16.23\times 10^{-5}g.

Solution : Given,

pH = 8.94

Volume of solution = 380 ml = 380\times 10^{-3}      (1ml=10^{-3}L)

Molar mass of sulfuric acid = 98.079 g/mole

As we know,

pH+pOH=14\\pOH=14-8.94=5.06

pOH=-log[OH^-]

5.06=-log[OH^-]

[OH^-]=0.00000871=8.71\times 10^{-6}mole/L

Now we have to calculate the moles of OH^-.

Formula used : Moles=Concentration\times Volume

\text{ Moles of }[OH^-]=\text{ Concentration of }[OH^-]\times Volume\\\text{ Moles of }[OH^-]=(8.71\times 10^{-6}mole/L)\times (380\times 10^{-3}L)=3309.8\times 10^{-9}moles

For neutralization, equal number of moles of H^+ ions will neutralize same number of OH^- ions.

\text{ Moles of }[OH^-]=\text{ Moles of }[H^+]=3309.8\times 10^{-9}moles

As, H_2SO_4\rightarrow 2H^++SO^{2-}_4

From this reaction, we conclude that

2 moles of H^+ ion is given by the 1 mole of H_2SO_4

3309.8\times 10^{-9} moles of H^+ ion is given by \frac{3309.8\times 10^{-9}}{2}=1654.9\times 10^{-9} moles of H_2SO_4

Now we have to calculate the mass of sulfuric acid.

Mass of sulfuric acid = Moles of H_2SO_4 × Molar mass of sulfuric acid

Mass of sulfuric acid = (1654.9\times 10^{-9}moles)\times (98.079g/mole)=162310.94\times 10^{-9}=16.23\times 10^{-5}g

Therefore, the mass of sulfuric acid needed is 16.23\times 10^{-5}g.

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3 years ago
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What occurs to the atoms of reactants in a chemical reaction?

Answer:

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