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3 years ago

Please help

Chemistry

2 answers:

lina2011 [118]3 years ago

7 0

Answer:

The warmer, lighter air rises, bringing cooler, heavier air to low altitudes.

Air at higher altitudes doesn't have as much air weighing down on it from above.

Explanation:

In short - air pressure is the result of the cumulative force that air molecules act on objects below them due to Earth's gravity. The higher the altitude, the less air molecules there are to act a force below them, and therefore, there's less air pressure at higher altitudes.

kotykmax [81]3 years ago

3 0

Answer:

I believe it's the second option "Lighter air molecules float above heavier air molecules

Explanation:

I believe this because as altitude increases the amount of gas molecules decrease which makes the air less dense

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What happens in the artificial transmutation of an element? Include an example.

Mice21 [21]

What happens in the artificial transmutation is that the nucleous is bombarded with high energy particles which we can describe as kinetic energy and the idea for them is to induce what we call transmutation. Also what happens is that the high energy particles are accelerated. One of the examples is when nitrogen is transformed into hydrogen by combining its nucleous with an alpha particle

6 0

3 years ago

The [H+] is 0.001 M. What is the pH?

galina1969 [7]

Hopes this helps:

Answer: So the pH of the solution is 4.

7 0

3 years ago

Calculate the molarity of 8.42 x 102 mL of solution containing 22.4 g of potassium iodide.

givi [52]

Answer:

Molarity = 0.154 M

Explanation:

Given data:

Volume of solution = 8.42 × 10² mL ( 8.42 × 10² /1000 = 0.842 L)

Mass of potassium iodide = 22.4 g

Molarity of solution = ?

Solution:

Number of moles of potassium iodide:

Number of moles = mass/molar mass

Number of moles = 22.4 g/ 166.0 g/mol

Number of moles = 0.13 mol

Molarity:

Molarity = number of moles / volume in L

Molarity = 0.13 mol / 0.842 L

Molarity = 0.154 M

8 0

3 years ago

A chemistry student needs 10.0g of ethanolamine for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the

iogann1982 [59]

Answer: The volume of ethanolamine the student should pour out is $9.80cm^3$

Explanation:

To calculate the volume of ethanolamine we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Density of ethanolamine = $1.02g/cm^3$

Mass of ethanolamine = 10.0 g

Volume of ethanolamine = ?

Putting values in above equation, we get:

$1.02g/cm^3=\frac{10.0g}{\text{Volume of ethanolamine}}\\\\{\text{Volume of ethanolamine}=\frac{10.0g}{1.02g/cm^3}=9.80cm^3$

Thus the volume of ethanolamine the student should pour out is $9.80cm^3$

4 0

4 years ago

determine the empirical and molecular formula of a compound composed of 18.24 g carbon, 0.51 g hydrogen, and 16.91 g fluorine an

Vika [28.1K]

Answer: The empirical formula for the given compound is $C_3HF_2$ and molecular formula for the given compound is $C_{24}H_8F_{16}$

Explanation : Given,

Mass of C = 18.24 g

Mass of H = 0.51 g

Mass of F = 16.91 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{18.24g}{12g/mole}=1.52moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.51g}{1g/mole}=0.51moles$

Moles of Fluorine = $\frac{\text{Given mass of Fluorine}}{\text{Molar mass of Fluorine}}=\frac{16.91g}{19g/mole}=0.89moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.51 moles.

For Carbon = $\frac{1.52}{0.51}=2.98\approx 3$

For Hydrogen = $\frac{0.51}{0.51}=1$

For Fluorine = $\frac{0.89}{0.51}=1.74\approx 2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : F = 3 : 1 : 2

The empirical formula for the given compound is $C_3H_1F_2=C_3HF_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

We are given:

Molar mass = 562.0 g/mol

Mass of empirical formula = 3(12) + 1(1) + 2(19) = 75 g/eq

Putting values in above equation, we get:

$n=\frac{562.0}{75}=7.49\approx 8$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_3HF_2=(C_3HF_2)_n=(C_3HF_2)_8=C_{24}H_8F_{16}$

Thus, the molecular formula for the given compound is $C_{24}H_8F_{16}$

8 0

3 years ago