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3 years ago

In two or more complete sentences, describe the process of fractional distillation that used to refine crude oil.

Chemistry

2 answers:

Oksi-84 [34.3K]3 years ago

3 0

I hope this helps you

postnew [5]3 years ago

3 0

Answer:

heated crude oil enters a tall fractionating column , which is hot at the bottom and gets cooler towards the top.

vapours from the oil rise through the column.

vapours condense when they become cool enough.

liquids are led out of the column at different heights.

sorry for bad spelling i think this is right

hope this helps :)

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An OH group attached to a hydrocarbon is called a _________ group whereas ______________ is a polyatomic ion with a charge of __

rodikova [14]

Answer:

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3 years ago

Calculate the mass of arsenic trihydride produced from 117.4 g of hydrogen gas with excess arsenic trioxide:

Lana71 [14]

Answer: The mass of $AsH_3$ produced is, 1528.8 grams.

Explanation : Given,

Mass of $H_2$ = 117.4 g

Molar mass of $H_2$ = 2 g/mol

First we have to calculate the moles of $H_2$ .

$\text{Moles of }H_2=\frac{\text{Given mass }H_2}{\text{Molar mass }H_2}$

$\text{Moles of }H_2=\frac{117.4g}{2g/mol}=58.7mol$

Now we have to calculate the moles of $AsH_3$

The balanced chemical equation is:

$6H_2+As_2O_3\rightarrow 2AsH_3+3H_2O$

From the reaction, we conclude that

As, 6 moles of $H_2$ react to give 2 moles of $AsH_3$

So, 58.7 moles of $H_2$ react to give $\frac{2}{6}\times 58.7=19.6$ mole of $AsH_3$

Now we have to calculate the mass of $AsH_3$

$\text{ Mass of }AsH_3=\text{ Moles of }AsH_3\times \text{ Molar mass of }AsH_3$

Molar mass of $AsH_3$ = 78 g/mole

$\text{ Mass of }AsH_3=(19.6moles)\times (78g/mole)=1528.8g$

Therefore, the mass of $AsH_3$ produced is, 1528.8 grams.

6 0

3 years ago

Please help asappp‍♀️!

solniwko [45]

Can you show me the passage?

6 0

3 years ago

Read 2 more answers

How many grams are there in 3.5 moles of H20

aksik [14]

Molar mass H₂O = 18.0 g/mol

1 mol ----- 18.0 g
3.5 moles --- ?

Mass ( H₂O) = 3.5 x 18.0 / 1

=> 63.0 g

hope this helps!

8 0

4 years ago

Nitric oxide can be oxidized in air to form nitrogen dioxide. At normal atmospheric concentrations this is a very slow process.

lawyer [7]

Answer:

exothermic

Explanation:

This is an exothermic reaction because you can see the 232.4 kJ at the end of the reaction. That means that 232.4 kilo-joules are released when the reaction happens; when energy is released during a reaction, the reaction is exothermic.

Tell me if you need anything else! :)

6 0

4 years ago