Explain the kinetic energy of the particles in each of the 3 main states of matter.

The raw water supply for a community contains 18 mg/L total particulate matter. It is to be treated by addition of 60 mg alum (A

s344n2d4d5 [400]

Solution :

Given :

The steady state flow = 8000 $m^3 /d$

$= 80 \times 10^5 \ I/d$

The concentration of the particulate matter = 18 mg/L

Therefore, the total quantity of a particulate matter in fluid $= 80 \times 10^5 \ I/d \times 18 \ mg/L$

$= 144 \times 10^6 \ mg/g$

$= 144 \ kg/d$

If 60 mg of alum $[Al_2(SO_4)_3.14 H_2O]$ required for one litre of the water treatment.

So Alum required for $80 \times 10^5 \ I/d$

$= 80 \times 15^5 \ I/d \times 60 \ mg \ alum /L$

$= 480 \times 10^6 \ mg/d$

or 480 kg/d

Therefore the alum required is 480 kg/d

1 mg of the alum gives 0.234 mg alum precipitation, so 60 mg of alum will give $= 60 \times 0.234 \text{ of alum ppt. per litre}$

$= 14.04$ mg of alum ppt. per litre

480 kg of alum will give = 480 x 0.234 kg/d

= 112.32 kg/d ppt of alum

Daily total solid load is $= 144 \ kg/d + 112.32 \ kg/d$

= 256.32 kg/d

So, the total concentration of the suspended solid after alum addition $= 18 \ mg/L + 60 \times 0.234$

= 32.04 mg/L

Therefore total alum requirement = 480 kg/d

b). Initial pH = 7.4

The dissociation reaction of aluminium hydroxide as follows :

$Al(OH)_3 \rightleftharpoons Al^{3+} + 3OH^{-}$

After addition, the aluminium hydroxide pH of water will increase due to increase in $OH^-$ ions.

Therefore, the pH of water will be acceptable range after the addition of aluminium hydroxide.

c). The reaction of $CO_2$ and water as follows :

$CO_2 (g) + H_2O (l) \rightarrow H_2CO_3$

For the atmospheric pressure :

$p_{CO_2} = 3.5 \times 10^{-4} \ atm$

And the pH is reduced into the range of 5.9 to 6.4

6 0

3 years ago

Use convection in a sentence

Vinil7 [7]

Convection

Convection is when heat is transferred by mass motion of a fluid.

6 0

4 years ago

PLEASE ANSWER Which is/are true?

Alona [7]

You have to check each statement, so this is equivalent to 5 different questions.

Answers:

The true statements are:

b. Si has valence electrons in the n = 3 energy level.

d. Xe has valence electrons in the n = 5 energy level.

Explanations:

a. Li has valence electrons in the n = 1 energy level.

Answer: False.

Valence electrons are the electrons in the outermost main energy level (shell of electrons).

To determine where the valence electrons are, you build the electron configuration, using Aufbau rules to predict the orbital filling: in increasing order of energy.

The atomic number of lithium (Li) is 3. Hence, you have to distribute 3 electrons, and so its electron confiuration is:

1s² 2s¹

The only valence electron is in the 2s orbital, i.e. in the n = 2 energy level.

b. Si has valence electrons in the n = 3 energy level.

Answer: True

Silicon (Si) has atomic number 14, so you have to distribute 14 electrons in increasing order of energy:

1s² 2s² 2p⁶ 3s² 3p²

Thus, Si has five valence electrons, and they are in the n = 3 energy level.

c. Ga has valence electrons in the n = 3 energy level.

Answer: False

Gallium has atomic number 31, so you have to distribute 31 electrons, filling the orbitals in increasing order of enery.

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹

The highest energy level is 4. This is where the valence electrons are. So, Ga has the valence electrons in the n = 4 level (not n = 3 as the statement describes).

d. Xe has valence electrons in the n = 5 energy level.

Answer: True

The atomic number of Xe is 54.

Using the short notation (noble gas notation), and filling the orbitals in increasing order of energy, you get the configuration:

[Kr] 5s² 4d¹⁰ 5p⁶.

Hence, the valence electrons are in the n ) 5 level, such as the statement describes.

e. P has valence electrons in the n = 2 energy level.

Answer: False

Phosphorus (P) has atomic number 15, hence there are 15 electrons.

The electron configuration following the increasing order of energy, which you can remember using Aufbau rules, is:

1s² 2s² 3s² 3p³

Then, the valence electrons are in the n = 3 energy level; not in the n = 2 energy level.

3 0

3 years ago

An isotope of which element has an atomic number of 6 and a mass number of 14

attashe74 [19]

Carbon-14 radioactive isotope

4 0

3 years ago

Read 2 more answers

study the diagram and answer the following questions. a. Name A and B. b. Which element is it? Write its name and B symbol. p*=

Oksana_A [137]

Ai. A is called nucleus

Aii. B is called electron shell

B. The name of the element is Neon and the symbol of the element is Ne.

Ci. The atomic mass of the element is 20.

Cii. The atomic number of the element is 10

Di. The element belongs to group 18.

Dii. The element belongs to period 2.

E. The element has a valency of 8

A. Determination of the name of A and B

In the diagram given above, A is called the nucleus because it contains the neutrons and the protons of the atom.

B is called the electron shell because it contains the electrons of the atoms

B. Determination of the name and symbol of the element.

From the diagram given above,

The element has 10 protons. This simply means that the atomic number of the element is 10.

Comparing the atomic number of the element with those in the periodic table, the element is Neon with a symbol of Ne.

C. Determination of the atomic mass and atomic number.

Ci. Determination of the mass number

Proton = 10

Neutron = 10

<h3>Mass number =?</h3>

Mass number = Proton + Neutron

Mass number = 10 + 10

<h3>Mass number = 20</h3>

Thus, the atomic mass of the element is 20.

Cii. Determination of the atomic number.

The atomic number of an element is simply the number of protons in the atom of the element.

Proton = 10

Therefore,

Atomic number = proton = 10

Thus, the atomic number of the element is 10

D. Determination of the group and period.

Di. The group to which an element belongs to can be obtained by simply calculating the number of electrons in the outermost shell of the atom.

From the diagram given above, the outermost shell has 8 electrons. This suggest that the element has completely filled outermost shell.

Therefore, the element belongs to group 18 (i.e the noble gas)

Dii. The number of electron shell talks about the period to which and element belongs to.

From the diagram given above, the element has 2 electron shells.

Therefore, the element belongs to period 2

E. Determination of the valence electron(s)

The valence electron(s) is the number of electrons in the outermost shell of the atom.

From the diagram given above,

The outermost shell has 8 electrons.

Therefore, the element has 8 valence electrons

Learn more: brainly.com/question/5352570

3 0

2 years ago