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3 years ago

After chlorofluorocarbons we’re banned, which class of chemicals was used in their place

Chemistry

2 answers:

Damm [24]3 years ago

8 0

Answer:

Hydrofluorocarbons

Explanation:

Law Incorporation [45]3 years ago

3 0

Answer:

Hydrofluorocarbons

Explanation:

Earlier chlorofluorocarbons were used for refrigeration purpose. But they were banned as they were primary cause of ozone depletion.

In order to replace chlorofluorocarbons, now hydrofluorocarbons are used which helps to protect earth from stratospheric ozone-depleting substances.

The difference between chlorofluorocarbons and hydrofluorocarbons is of hydrogen. In hydrofluorocarbons one of the halogen is being replaced by hydrogen.

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Sulfur and oxygen form both sulfur dioxide and sulfur trioxide. When samples of these were decomposed the sulfur dioxide produce

Zinaida [17]

Answer : The mass of oxygen per gram of sulfur for sulfur dioxide and sulfur trioxide is, 0.997 g and 1.5 g respectively.

Explanation : Given,

Mass of oxygen in sulfur dioxide = 3.49 g

Mass of sulfur in sulfur dioxide = 3.50 g

Mass of oxygen in sulfur trioxide = 9.00 g

Mass of sulfur in sulfur trioxide = 6.00 g

Now we have to calculate the mass of oxygen per gram of sulfur for sulfur dioxide and sulfur trioxide.

Mass of oxygen per gram of sulfur for sulfur dioxide = $\frac{\text{Mass of oxygen}}{\text{Mass of sulfur}}$

Mass of oxygen per gram of sulfur for sulfur dioxide = $\frac{3.49}{3.50}=0.997g$

and,

Mass of oxygen per gram of sulfur for sulfur trioxide = $\frac{\text{Mass of oxygen}}{\text{Mass of sulfur}}$

Mass of oxygen per gram of sulfur for sulfur trioxide = $\frac{9.00}{6.00}=1.5g$

Thus, the mass of oxygen per gram of sulfur for sulfur dioxide and sulfur trioxide is, 0.997 g and 1.5 g respectively.

8 0

3 years ago

Pick 3 objects around your room and write 2 observations and 2 interpretations about object . BTW I just moved I only have a bed

Katen [24]

Walls, floors, bed, door, doorknob. You have options

6 0

2 years ago

Beryllium oxide, Beo, is an electrical insulator. How

egoroff_w [7]

Answer:

There are 10.0 moles of beryllium oxide in a 250 grams sample of the compound.

Explanation:

We can calculate the number of moles (η) of BeO as follows:

$\eta = \frac{m}{M}$

Where:

m: is the mass = 250 g

M: is the molar mass = 25.0116 g/mol

Hence, the number of moles is:

$\eta = \frac{250 g}{25.0116 g/mol} = 10.0 moles$

Therefore, there are 10.0 moles of beryllium oxide in a 250 grams sample of the compound.

I hope it helps you!

3 0

2 years ago

Chemistry Conversion

kvv77 [185]

Answer:

Explanation:

193.02 times 9.55 it's going to be 1843.341

9.55= 191.20 milli

4 0

2 years ago

What are the respective concentrations (m) of fe3+ and i- afforded by dissolving 0.200 mol fei3 in water and diluting to 725 ml?

Natalka [10]

Molarity = moles / liter of solution

Given, Moles of Fe³⁺ = 0.200

Volume of solution = 725 ml = 0.725 L

Conversion factor: 1000 ml = 1L

Molarity = 0.200 / 0.725 L = 0.275 M

The dissociation of Fel₃ in water is ad follows:

Fel₃ → Fe³⁺ + 3l⁻

1 mole of Fel₃ gives 1 mole of Fe³⁺ ions and 3 moles of l⁻

Since the solution is 0.275 M of Fel₃, so there are 0.275 M of Fe³⁺ ions,

and (3 x 0.275 M) = 0.825 M of l⁻ ions.

7 0

3 years ago