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3 years ago

The two factors that are most important in determining the density of air are:

Chemistry

2 answers:

Pie3 years ago

8 0

Answer:

c. temperature and water vapor content.

Explanation:

The density of any substance is dependent of temperature, and in gases, the variations is greater than in any other substance, therefore, temperature is very important to calculate air density. Also, the concentration of water vapor in the air can vary depending where is located, and that concentration will affect the density because it affects the average mass of air.

Thepotemich [5.8K]3 years ago

8 0

Answer:

c. temperature and water vapor content is the correct answer.

Explanation:

temperature and water vapor content are the two most important in determining the density of air.

When the temperature gets increase it results in the increase of volume and density gets decreases.

Temperature is an important factor to determine the air density.

The concentration of water vapor in the air change depending on where it is placed and so when water vapor is added it will change the density of air because it changes the average mass of air and density gets decrease.

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An acid with molar mass 84.48 g/mol is titrated with 0.650 M KOH. What volume of KOH solution is needed to titrate 1.70 grams of

RSB [31]

Answer:

$V=0.0310L=3.10mL$

Explanation:

Hello.

In this case, since the acid is monoprotic and the KOH has one hydroxyl ion only, we can see that at the equivalence point the moles of both of them are the same:

$n_{acid}=n_{KOH}$

Thus, since we are given 1.70 g of the acid, we compute the moles of acid that were titrated:

$n_{acid}=1.70g*\frac{1mol}{84.48g}=0.0201mol$

Which equal the moles of KOH. In such a way, since the molarity is defined as moles over liters (M=n/V), the liters are moles over molarity (V=n/M), thus, the resulting volume is:

$V=\frac{0.0201mol}{0.650mol/L}\\\\V=0.0310L=3.10mL$

Best regards!

7 0

3 years ago

A theory should be able to explain the relevant data and lead to correct predictions.

olya-2409 [2.1K]

The correct answer is true

5 0

3 years ago

Read 2 more answers

What is the net ionic equation of the reaction of FeCl2 with NaOH? Express you answer as a chemical equation including phases.

Lilit [14]

Answer:

Fe²⁺(aq) + 2OH⁻(aq) → Fe(OH)₂(s)

Explanation:

To determine the reaction, we define the reactants:

FeCl₂, NaOH

We dissociate them:

FeCl₂(aq) → Fe²⁺(aq) + 2Cl⁻ (aq)

NaOH (aq) → Na⁺ (aq) + OH⁻(aq)

Salts from chloride are soluble, except for Ag⁺, Pb²⁺, Hg₂²⁺, Cu⁺

The OH⁻ and the Fe²⁺ bonds to make a precipitate.

So, the molecular complete equation is:

FeCl₂(aq) + 2NaOH(aq) → Fe(OH)₂(s) ↓ + 2NaCl(aq)

When we dissociate the elements, we get the net ionic equation but as we produced an state's change, the compound stays the same.

We cancel the spectators ions (the ones, that are repeated)

Fe²⁺(aq) + 2Cl⁻ (aq) + 2Na⁺ (aq) + 2OH⁻(aq) → Fe(OH)₂(s) + 2Na⁺(aq) + 2Cl⁻(aq)

Fe²⁺(aq) + 2OH⁻(aq) → Fe(OH)₂(s)

5 0

3 years ago

If 20.00 moles of KClO3 react, how many molecules of O2 will form?

Tanzania [10]

Answer:

Explanation:

2KClO₃ = 2KCl + 3O₂

2 moles of potassium chlorate gives 3 moles of oxygen gas

20 moles of potassium chlorate will give 30 moles of oxygen gas .

30 moles of oxygen = 30 x 6.02 x 10²³ molecules of oxygen .

= 180.6 x 10²³ molecules of O₂ .

6 0

3 years ago

If oxygen has a molar mass of 16.0 g/mole, carbon has a molar mass of 12.0 g/mole and hydrogen has a molar mass of 1.01 g/mole,

Stolb23 [73]

The number of mole of ethanol present in the beaker is 0.217 mole

Description of mole
The mole of a substance is related to it's mass and molar mass according to the following equation:
Mole = mass / molar mass

How to determine the mole of C₂H₅OH
From the question given above, the following data were obtained:
Mass of C₂H₅OH = 10 g
Molar mass of C₂H₅OH = (12×2) + (1.01×5) + 16 + 1.01 = 46.06 g/mol
Mole of C₂H₅OH =?

Mole = mass / molar mass
Mole of C₂H₅OH = 10 / 46.06
Mole of C₂H₅OH = 0.217 mole

Learn more about mole:
brainly.com/question/13314627

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5 0

2 years ago