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wolverine [178]
3 years ago
14

The temperature of 200 mL of gas

Chemistry
1 answer:
Elden [556K]3 years ago
6 0

Answer:

691.6 torr

Explanation:

Given data:

Initial temperature = 273 K

Initial pressure = 1 atm

Final temperature = -25 °C (-25 + 273 = 248 k)

Final pressure = ?

Solution:

P₁/T₁ = P₂/T₂

P₁ = Initial pressure

T₁ = Initial temperature

P₂ = Final pressure  

T₂ = Final temperature

Now we will put the values in formula.

P₁/T₁ = P₂/T₂

P₂ = P₁T₂/T₁  

P₂ = 1 atm × 248 K / 273 k

P₂ =248  atm. K / 273 K

P₂ = 0.91 atm  

In torr:

0.91  × 760 = 691.6 torr

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Empirical Formula = ?

Solution

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Empirical formula is the simplest ration of atoms in the molecule but not all numbers of atoms in a compound.

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tha ration of the molecular formula should be divided by whole number to get the simplest ratio of molecule

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Now

Look at the ratio of these two atoms in the compound

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                         8 : 8

Divide the ratio by two to get simplest ratio

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What is the direction of the polarity of the indicated bond in h3c−oh marked by δ+ and δ−?
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Oxygen is more electron negative than carbon. So, being more electron negative, the bonding electrons are more towards oxygen and it cases partial negative charge on oxygen and partial positive charge on carbon. The direction of the polarity is from less electron negative carbon to more electron negative oxygen.

It is shown in the diagram below:


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