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boyakko [2]
3 years ago
13

How to find the mass of 12dm³ of hydrogen, H2

Chemistry
1 answer:
Soloha48 [4]3 years ago
5 0

you can use the formula F=MA to find any mass of almost anything .

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(58 g)/ (4L) reduce units to one
katen-ka-za [31]

Answer is 14.5 g L⁻¹.

<em>Explanation;</em>

Here, the question says reduce the units as one.

The presented units are g/L. To reduce the units to one, what we can do is take L to the upper side.

This can be done according to the rules of indices;

1 / aˣ = a⁻ˣ

Like that, we can write 1 / L as L⁻¹.

Hence, the reduced unit is g L⁻¹.

But remember to keep a space between when writing two different units.

Actually, this is an unit for density.

3 0
3 years ago
Metals tend to ________ electrons and form _______ ions.
masya89 [10]
<span>Metals tend to lose electrons and form electro-positive ions / cations.</span>
5 0
3 years ago
A mixture of 15.0 g of the anesthetic halothane (C2HBrClF3 197.4 g/mol) and 22.6 g of oxygen gas has a total pressure of 862 tor
AlexFokin [52]

Answer : The partial pressure of C_2HBrClF_3 and O_2 are, 84 torr and 778 torr respectively.

Explanation : Given,

Mass of C_2HBrClF_3 = 15.0 g

Mass of O_2 = 22.6 g

Molar mass of C_2HBrClF_3 = 197.4 g/mole

Molar mass of O_2 = 32 g/mole

First we have to calculate the moles of C_2HBrClF_3 and O_2.

\text{Moles of }C_2HBrClF_3=\frac{\text{Mass of }C_2HBrClF_3}{\text{Molar mass of }C_2HBrClF_3}=\frac{15.0g}{197.4g/mole}=0.0759mole

and,

\text{Moles of }O_2=\frac{\text{Mass of }O_2}{\text{Molar mass of }O_2}=\frac{22.6g}{32g/mole}=0.706mole

Now we have to calculate the mole fraction of C_2HBrClF_3 and O_2.

\text{Mole fraction of }C_2HBrClF_3=\frac{\text{Moles of }C_2HBrClF_3}{\text{Moles of }C_2HBrClF_3+\text{Moles of }O_2}=\frac{0.0759}{0.0759+0.706}=0.0971

and,

\text{Mole fraction of }O_2=\frac{\text{Moles of }O_2}{\text{Moles of }C_2HBrClF_3+\text{Moles of }O_2}=\frac{0.706}{0.0759+0.706}=0.903

Now we have to partial pressure of C_2HBrClF_3 and O_2.

According to the Raoult's law,

p^o=X\times p_T

where,

p^o = partial pressure of gas

p_T = total pressure of gas

X = mole fraction of gas

p_{C_2HBrClF_3}=X_{C_2HBrClF_3}\times p_T

p_{C_2HBrClF_3}=0.0971\times 862torr=84torr

and,

p_{O_2}=X_{O_2}\times p_T

p_{O_2}=0.903\times 862torr=778torr

Therefore, the partial pressure of C_2HBrClF_3 and O_2 are, 84 torr and 778 torr respectively.

6 0
3 years ago
How fast did the universe expand?​
Sidana [21]

Answer:

Actually there is no answer but there is so much theories but people mostly says Bug Bang

7 0
3 years ago
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How is iron extracted? Describe in brief​
Feliz [49]

Answer:Iron is extracted from iron ore in a huge container called a blast furnace. Iron ores such as haematite contain iron(III) oxide, Fe 2O 3. The oxygen must be removed from the iron(III) oxide in order to leave the iron behind. Reactions in which oxygen is removed are called reduction reactions.

3 0
3 years ago
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