What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a solution to a volume of

Answer:

b. because its Rigel star

Explanation:

hope itsattachments

Answer:

D

Explanation:

Protons and Neutrons both have a mass of about 1 amu so you add them but electrons have a mass of 0 amu so they are left out.

Answer:

mezcla homogénea

Answer:

heterogeneous mixture

Explanation:

you can split the mixture easily with you hands while homogeneous mixtures is dissolved

Answer:

It's option a) Permeability.

Answer:

2) To find the atoms from the moles, you just multiply Avogadro's number (6.02 x 10^23) by the moles.

So 3.35 x (6.02 x 10^23) = 2.0167 x 10^24 atoms are in 3.35 moles of aluminum

3) If the question is asking under standard temperature and pressure, we know that if we divide the volume by the molar volume of a gas (which is 22.7 in standard temperature and pressure), we can get the moles.  

So 101.25L / 22.7 = 4.46 mol

4) We know that to find the moles, it is the mass divided by the molar mass. If we rearrange the equation to solve for mass, we have to multiply the moles by the molar mass to get there.

Nitrogen's (N) molar mass on the periodic table is 14g/mol, but since Nitrogen is a diatomic element, it would be N2 by itself. So multiply 14 by 2, which will give you 28g/mol. N2's molar mass is 28g/mol.

Now you multiply 13.7 moles by 28g/mol, which will give you 383.6g

Just did a few edits here, 4.46 for question 3 is in moles not L

Taking into account the definition of avogadro's number,

2. 3.35 moles of aluminum contains 2.018ײ⁴ atoms.

3. 4.52 moles of CO₂ gas are in a 101.25 L container filled with CO₂ gas.

4. 13.7 moles of N₂ contain 383.6 grams.  

Avogadro's Number is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023×10²³ particles per mole. Avogadro's number applies to any substance.

Then you can apply the following rule of three: if 1 mole of aluminum contains 6.023×10²³ atoms, then 3.35 moles of aluminum contains how many atoms?

amount of atoms of aluminum= (6.023×10²³ atoms × 3.35 moles)÷ 1 mole

amount of atoms of aluminum=2.018ײ⁴ atoms

Finally, 3.35 moles of aluminum contains 2.018ײ⁴ atoms.

The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.

Then, you can apply the following rule of three: If by definition of the STP conditions 1 mole of CO₂ occupies a volume of 22.4 L, how many moles does 101.25 L occupy?

[tex]amount of moles of CO_{2} =\frac{101.25 Lx1 mole of CO_{2} }{22.4 L}[/tex]

amount of moles of CO₂= 4.52 moles

4.52 moles of CO₂ gas are in a 101.25 L container filled with CO₂ gas.

The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.

In this case, the molar mass of N₂ is 28 g/mole. So, you can apply the following rule of three:  If 1 mole of N₂ contains 28 grams, 13.7 moles of N₂ contain how much mass?

[tex]mass=\frac{13.7 moles x28 grams}{1 mole}[/tex]

mass= 383.6 grams

13.7 moles of N₂ contain 383.6 grams.

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Answer:

It will be a covalent bond.

Explanation:

When two atoms combine, the difference between their electronegativities is an indication of the type of bond that will form. If the difference between the electronegativities of the two atoms is small, neither atom can take the shared electrons completely away from the other atom and the bond will be covalent.

Gravitational Potential energy:

The Gravitational potential energy of

an object at a point above the ground

is defined as the work done in raising

it from the ground to that point against

gravity.

Consider an object of mass "m" is raised

to heighth from the ground.

A force is required to do this. the

minimum force required to raise the

object is equal to the weight of the

object[mg]

The object gains energy equal to the

work done on it. Let the work done on

the object against gravity be "w"

WorkDone=W= Force x displacement

=mgxh

..W=mgh

since the workdone on the object is

equal to "mgh" an energy equal to "mgh"

units is gained by object.This is the

potential energy of object at height "h"

.. P.E=mgh

Answer:

The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid.  

Explanation:

The stronger the acid, the weaker its conjugate base and vice versa  A very weak acid has a very strong conjugate base.

When 1-bromo propane is reacted with sodium metal, the propane and sodium bromide are formed.

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C9H8O. .....................

Answer:

a

Explanation:

Answer:

Im pretty sure it's B, almost 100% sure

Explanation:

A. iron

B. iodine

C. Helium

D. calcium

E. lead

F. hydrogen

check your periodic table to see if they are correct

atomic number, proton number and electron are the same

to find neutron = mass number - atomic number

Finding molar mass of NaOH

We know that

Molar mass of Sodium (Na) = 23 g/mol

Molar mass of Oxygen (O) = 32 g/mol

Molar mass of Hydrogen (H) = 2 g/mol

So,

Mass of 1 mole of NaOH

=> 1 × 23 + 1 × 16 + 1 × 1

=> 23 + 16 + 1

=> 40 g/mol

Now,

Mass = 40 × 0.25

Mass = 10 g

The boiling point of salt water is greater than that of fresh water hence the electrostatic forces between molecules in salt water is greater than that between the molecules in salt water.

Fresh water contains does not contain dissolved solutes like salt water. Salt water contains a lot of dissolved mineral salts making the salt water to be rich in ions.

Generally, the boiling points of substances can serve as a measure of the strength of electrostatic forces between molecules in either kind of water. We will easily find the that the boiling point of salt water is far higher than that of fresh water indicating greater electrostatic forces between molecules in salt water than between molecules in fresh water.

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The strongest intermolecular bonding in ethanol is hydrogen bonding.

Intermolecular forces are the forces that hold two molecules of a substance together in a given state of matter. For ethanol, the strongest intermolecular force is hydrogen bonding.

Hydrogen bonding occurs when hydrogen is directly linked to a highly electronegative element such as oxygen, nitrogen, fluorine or sulfur. The existence of intermolecular hydrogen bonds accounts for unusual properties such as abnormally high melting and boiling points.

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Answer:

92.01 g/mol

Explanation:

So first you need to find the empirical formula by the percents. That would be, assuming that you have 100 grams of the the sample, divide each quantity of each element found by its respective molar mass.

30.4 g of N ÷ 14 g/mol N= 2.17 mol of N

69.6 g of O ÷ 16g/mol= 4.35 mol of O

You can establish now the empirical formula.

N2.17O4.35,

but since you can't have a decimal subscript, you divide each subscript by the minimum subscript

NO2

So then you're said that the molecular formula derived from that empirical formula has 2 nitrogen, so you multiply all the subscripts, by 2:

N2O4

-Dinitrogen Tetraoxide

-Nitrogen oxide (IV)

Then all you have to do is find the molecular mass of the compound using the periodic table and what you obtain is the molar mass.

remember: molecular mass is correspondent to molar mass.

Answer:

[tex] \huge{5.632 \times {10}^{ - 19} \: J}[/tex]

Explanation:

The energy of the proton can be found by using the formula

where

E is the energy in J

f is the frequency in Hz

h is the Planck's constant which is

6.626 × 10-³⁴ Js

From the question we have

E = 6.626 × 10-³⁴ × 8.5 × 10¹⁴

We have the final answer as

[tex]5.632 \times {10}^{ - 19} \:J[/tex]

Hope this helps you

Answer:

To make H2O, you need two H and one O. in this equation, you are given two Os which is too many. you'll end up with an extra O. H2 + O2 -> H2O + O

Answer:

metal : Mercury(Hg)

non metal : bromine (Br)

Explanation:

mercury is liquid at room temperature and pressure and the same as bromine

Answer:

Mechanical Waves

Answer:

If you are given with the atomic number of an element you can find it's period number and group number. The period number is related to the number of electron occupied shells in the element and the period number is linked to its valence electrons.

Explanation:

hope it helps luv <3

The boiling points of two or three other pairs of liquids in which one liquid has a lower molecular mass than the other can be studied in order to see if the pattern is consistent.

The boiling point of a substance refers to the temperature at which its vapor pressure is equal to the atmospheric pressure. The boiling point of a substance has a lot to do with its molecular mass.

Generally, substances that has a higher molecular mass has a higher boiling point except other factors at at work. In order to confirm whether the pattern that you are noticing about molecular weights and boiling point is consistent, three other liquids with different molecular masses, one being higher than the other can be studied and their boiling points compared.

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Explanation:

Liquid-based lubricant

Answer:

study island : food service equipment

Explanation:

Answer:

Explanation:

Answer:

A

Explanation:

refer to textbook

Answer:

U shaped vallies?

Explanation:

(i dont know if this was one of the options)

The formula of trinitrogen tetrabromide is N3Br4

Trinitrogen features three molecules of nitrogen, N3

Tetrabromide features four molecules of bromide = Br4

Thus, the formula of trinitrogen tetrabromide is N3Br4

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The greenhouse gases are carbon dioxide, methane, and nitrous oxide.

The greenhouse effect has been defined as the entrapment of the sun's energy by the gases that result in the earth becoming warmer and a better place to live.

The gases present in the atmosphere that has been able to entrap the heat energy has been termed the greenhouse gases.

The greenhouse gases have been carbon dioxide, methane, and nitrous oxide.

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Answer:

carbon dioxide, nitrous oxide, methane

Explanation: