What type of weather is associated with high pressure?

What is the molariity of a 50.0 mL aqueous solution containing 10.0 grams of table salt, NaCl?

tia_tia [17]

Answer:

3 mol/L

Explanation:

You should know or have the equation to solve for Molarity which is;

M = n/v (M: Molarity) (n: moles of solute) (v: Liters of solute)

You can start off differently but I would start by converting the mL to L. This is your "v" value.

50.0 mL/ 1000 mL = 0.05 L

Now, you have to convert grams to moles in order to solve for molarity (M).

1.) On the periodic table find the molecular weights of Na and Cl.

Na= 22.99 g/mol Cl= 35.45g/mol

2.) Add them together to have their combined molecular weights.

22.99 + 35.45= 58.44 g/mol

3.) Now, you're going to use the "picket fence method" or whichever your teacher taught you to convert from grams to moles. This will be your "n" value. (I cannot show it on here without it looking weird, so my sincere apologies.)

10.0 g/ 58.44 g = 0.17111 mol

4.)You are now going to plug in your answers into the equation for Molarity.

M= 0.17111 mol / 0.05 L = 3.4222

5.) I am sure your professor might be a stickler so for sig figs sake when you multiply or divide use the smallest amount of sig figs you see which is 1. Round 3.4222 to 3 mol/L

Sorry this explanation is long let me know if you need a better more written out sample.

3 0

3 years ago

Maple syrup, which comes from the sap of maple trees, contains water and natural sugars. It’s a clear, brown liquid and the suga

jonny [76]

I would classify it as a homogeneous mixture that you can't see different particles in with a human eye but if you look through it in a microscope I would classify it as a heterogeneous mixture because you can see the different sugars and saps.Hope this helped???

3 0

3 years ago

Which of the following substances would be a good electrical conductor? A. KCl(s) B. C(s) C. Al(s) D. CO2(s)

finlep [7]

The correct answer would be B

8 0

3 years ago

Read 2 more answers

This is the weighted average of all of the isotopes of an element.

Darina [25.2K]

Answer:

Atomic mass

Explanation:

Atomic mass (Also called Atomic Weight, although this denomination is incorrect, since the mass is property of the body and the weight depends on the gravity) Mass of an atom corresponding to a certain chemical element). The uma (u) is usually used as a unit of measure. Where u.m.a are acronyms that mean "unit of atomic mass". This unit is also usually called Dalton (Da) in honor of the English chemist John Dalton.

It is equivalent to one twelfth of the mass of the nucleus of the most abundant isotope of carbon, carbon-12. It corresponds roughly to the mass of a proton (or a hydrogen atom). It is abbreviated as "uma", although it can also be found by its English acronym "amu" (Atomic Mass Unit). However, the recommended symbol is simply "u".

<u> The atomic masses of the chemical elements are usually calculated with the weighted average of the masses of the different isotopes</u> of each element taking into account the relative abundance of each of them, which explains the non-correspondence between the atomic mass in umas, of an element, and the number of nucleons that harbors the nucleus of its most common isotope.

In contrast, the atomic mass of an isotope does coincide approximately with the mass of its nucleons. This difference is due to the fact that the elements are not formed by a single isotope but by a mixture with certain abundances for each of them. While when we measure the mass of a particular isotope, we do not take abundance into account. In any case, not even the atomic mass of the isotopes equals the sum of the masses of the nucleons. This is due to mass defect.

7 0

3 years ago

Read 2 more answers

If 5.0 of al react with 9.0 g of O2, how many grams of Al2O3 (101.56 g/mol) can be formed

Law Incorporation [45]

<h3>Answer:</h3>

9.394 g of Al₂O₃

<h3>Explanation:</h3>

The reaction between Aluminium and Oxygen is given by the balanced equation;

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

We are given;

Mass of Aluminium as 5.0 g
Mass of Oxygen as 9.0 g

We are required to determine the mass of Al₂O₃ formed.

We are going to use the following simple steps;

<h3>Step 1: Calculate the number of moles of Aluminium and Oxygen </h3>

Moles = Mass ÷ Molar mass

Moles of Al;

Molar mass of Al = 26.98 g/mol

Moles of Al = 5.0 g ÷ 26.98 g/mol

= 0.185 moles

Moles of Oxygen gas

Molar mass of O₂ = 32.0 g/mol

Moles O₂ = 9.0 g ÷ 32.0 g/mol

= 0.28125 moles

From the equation, four moles of Aluminium reacts with three moles of oxygen gas.

Therefore, Aluminium is the rate limiting reagent while oxygen gas is in excess.

<h3>Step 2: Calculate the number of moles of Al₂O₃ formed </h3>

4 moles of Al reacts to produce 2 moles of Al₂O₃

Thus, the mole ratio of Al to Al₂O₃ is 2 : 1

Thus, moles of Al₂O₃ = Moles of Al ÷ 2

= 0.185 moles ÷ 2

= 0.0925 moles

<h3>Step 3: Calculate the mass of Al₂O₃ formed</h3>

Mass = Moles × Molar mass

Molar mass of Al₂O₃ is 101.56 g/mol

= 0.0925 moles ×101.56 g/mol

= 9.394 g

Therefore, the mass of Al₂O₃ formed is 9.394 g

6 0

3 years ago