Which option defines solute?

Write the chemical symbols for three different atoms or atomic anions with 36 electrons

Gekata [30.6K]

If you look at the periodic table, Krypton has an atomic number of 36. Krypton is one of the noble gases. They are a group of elements that are very stable because they obey the Octet Rule. As a result, other elements try to conform the electronic configurations of the nearest noble gases to them. They either give or take electrons in their valence shell.

The three atoms that have 36 electrons are: Kr (Krypton), Br⁻ (Bromide), and Rb⁺(Rubidium ion).

4 0

4 years ago

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How many liters are there in 144g of H₂O (g)?<br> What is the mass of 200L at STP of H₂O₂ (g)?

Lisa [10]

Answer:

1. 179.2 L

2. 303.62 g

Explanation:

1. Determination of volume of H₂O (g).

We'll begin by calculating the number of mole in 144 g of H₂O. This is illustrated below:

Mass of H₂O = 144 g

Molar mass of H₂O = (2×1) + 16 = 2 + 16 = 18 g/mol

Mole of H₂O =?

Mole = mass /Molar mass

Mole of H₂O = 144/18

Mole of H₂O = 8 moles

Finally, we shall determine volume of H₂O (g) as follow:

1 mole of any gas occupy 22.4L at stp.

Therefore, 8 moles of H₂O (g) will occupy =

8 × 22.4 = 179.2 L

Thus, 144 g of H₂O (g) occupies 179.2 L

2. Determination of the mass of H₂O₂ (g).

We'll begin by calculating the number of mole of H₂O₂ (g) that occupied 200 L at STP. this can be obtained as follow:

1 mole of any gas occupy 22.4 L at stp.

Therefore, Xmol of H₂O₂ (g) will occupy 200 L at STP i.e

Xmol of H₂O₂ (g) = 200/22.4

Xmol of H₂O₂ (g) = 8.93 moles

Thus, 8.93 moles of H₂O₂ (g) occupied 200 L at STP.

Finally, we shall determine the mass of H₂O₂ (g) as follow:

Mole of H₂O₂ (g) = 8.93 moles

Molar mass of H₂O₂ = (2×1) + (2×16) = 2 + 32 = 34 g/mol

Mass of H₂O₂ =?

Mole = mass /Molar mass

8.93 = mass of H₂O₂ /34

Cross multiply

Mass of H₂O₂ = 8.93 × 34

Mass of H₂O₂ = 303.62 g

5 0

3 years ago

Place the following substances in order of decreasing vapor pressure at a given temperature: BeF2, CH3OH, OF2?

Anit [1.1K]

Answer:

(b) BeF2 > OF2 > CH3OH

Explanation:

The degree and type of intermolecular forces present in a substance influences its vapour pressure considerably. The greater the magnitude and strength of intermolecular forces in the substance, the lower the vapour pressure of the substance.

BeF2 molecules are held together by weak vanderwaals forces hence BeF2 will exhibit the least degree of intermolecular interaction and have the highest vapour pressure. OF2 molecules are bound together by dipole interactions hence it will exhibit a lower vapour pressure compared to BeF2. CH3OH molecules form hydrogen bonds with water molecules hence it will exhibit the least vapour pressure among the trio.

3 0

3 years ago

A 1.00 l solution contains 3.50×10-4 m cu(no3)2 and 1.75×10-3 m ethylenediamine (en). the kf for cu(en)22+ is 1.00×1020. what is

Alik [6]

<span>Answer: A 1.00 L solution containing 3.00x10^-4 M Cu(NO3)2 and 2.40x10^-3 M ethylenediamine (en). contains 0.000300 moles of Cu(NO3)2 and 0.00240 moles of ethylenediamine by the formula Cu(en)2^2+ 0.000300 moles of Cu(NO3)2 reacts with twice as many moles of en = 0.000600 mol of en so, 0.00240 moles of ethylenediamine - 0.000600 mol of en reacted = 0.00180 mol en remains by the formula Cu(en)2^2+ 0.000300 moles of Cu(NO3)2 reacts to form an equal 0.000300 moles of Cu(en)2^2+ Kf for Cu(en)2^2+ is 1x10^20. so 1 Cu+2 & 2 en --> Cu(en)2^2+ Kf = [Cu(en)2^2+] / [Cu+2] [en]^2 1x10^20. = [0.000300] / [Cu+2] [0.00180 ]^2 [Cu+2] = [0.000300] / (1x10^20) (3.24 e-6) Cu+2 = 9.26 e-19 Molar since your Kf has only 1 sig fig, you might be expected to round that off to 9 X 10^-19 Molar Cu+2</span>

4 0

3 years ago

Apply the given electronegativities to each bond in the examples below to see which are polar and which are nonpolar. Multiple b

Nesterboy [21]

Answer:

H-O-H polar

O-C-O nonpolar

H-C-N polar

Explanation:

Looking up the electronegativities of the atoms involved in this question, we have:

Atom Electronegativity

H 2.2

C 2.55

N 3.04

O 3.44

All of the atoms differ in electronegativity resulting in individual dipole moments in H-O, O-C, H-C and C-N bonds. To find if the molecules will be polar we need to consider the structure of the compound to see if there is a resultant dipole moment.

In H-O-H, we have 2 lone pairs of electrons around the central oxygen atom which push the angle H-O-H of the ideal tetrahedral structure to be smaller than 109.5 º resulting in an overall dipole moment making it polar.

In O-C-O, we have two dipole moments that exactly cancel each other in the linear molecule since the central carbon atom does not have lone pairs of electrons since it has 2 double bonds. Therefore the molecule is nonpolar.

In H-C-N, again we have have a central carbon atom without lone pairs of electrons and the shape of the molecule is linear. But, now we have that the dipole moment in C-N is stronger than the H-C dipole because of the difference in electronegativity of nitrogen compared to hydrogen. The molecule has an overall dipole moment and it is polar.

8 0

3 years ago

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