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Monica [59]
3 years ago
13

An atom of argon has a radius rar = 88 pm and an average speed in the gas phase at 25°C of 172 m/s.

Chemistry
1 answer:
Rudik [331]3 years ago
7 0

Answer:

1.2* 10³ rNe.

Explanation:

Given speed of neon=350 m/s

Un-certainity in speed= (0.01/100) *350 =0.035 m/s

As per heisenberg uncertainity principle

Δx*mΔv ≥\frac{h}{4\pi }

4π

h

..................(1)

mass of neon atom =\frac{20*10^{-3} }{6.22*10^{-23} } =3.35*10^{-26} kg

6.22∗10

−23

20∗10

−3

=3.35∗10

−26

kg

substituating the values in eq. (1)

Δx =4.49*10^{-8}10

−8

m

In terms of rNe i.e 38 pm= 38*10^{-12}10

−12

Δx=\frac{4.49*10^{-8} }{38*10^{-12} }

38∗10

−12

4.49∗10

−8

=0.118*10^{4}10

4

* (rNe)

=1.18*10³ rN

= 1.2* 10³ rNe.

Explanation:

This is the answer

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Commercial hydrochloric acid (HCl) is typically labeled as being 38.0 % (weight %). The density of HCl is 1.19 g/mL. a) What is
Strike441 [17]

<u>Answer:</u>

<u>For a:</u> The molarity of commercial HCl solution is 12.39 M.

<u>For b:</u> The molality of commercial HCl solution is 16.79 m.

<u>For c:</u> The volume of commercial HCl solution needed is 2.42 L.

<u>Explanation:</u>

We are given:

Mass % of commercial HCl solution = 38 %

This means that 38 grams of HCl is present in 100 grams of solution.

To calculate the volume of solution, we use the equation:

Density=\frac{Mass}{Volume}

Density of HCl solution = 1.19 g/mL

Mass of solution = 100 g

Putting values in above equation:

1.19g/mL=\frac{100g}{\text{Volume of solution}}\\\\\text{Volume of solution}=84.034mL

  • <u>For a:</u>

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Molarity of solution = ?

Molar mass of HCl = 36.5 g/mol

Volume of solution = 84.034 mL

Mass of HCl = 38 g

Putting values in above equation, we get:

\text{Molality of commercial HCl solution}=\frac{38\times 1000}{36.5\times 84.034}\\\\\text{Molality of commercial HCl solution}=12.39M

Hence, the molarity of commercial HCl solution is 12.39 M.

  • <u>For b:</u>

To calculate the molality of solution, we use the equation:

Molarity=\frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}

Where,

m_{solute} = Given mass of solute (HCl) = 38 g

M_{solute} = Molar mass of solute (HCl) = 36.5 g/mol

W_{solvent} = Mass of solvent = 100 - 38 = 62 g

Putting values in above equation, we get:

\text{Molality of commercial HCl solution}=\frac{38\times 1000}{36.5\times 62}\\\\\text{Molality of commercial HCl solution}=16.79m

Hence, the molality of commercial HCl solution is 16.79 m.

  • <u>For c:</u>

To calculate the molarity of the diluted solution, we use the equation:

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of the concentrated solution

M_2\text{ and }V_2 are the molarity and volume of diluted solution

We are given:

M_1=6M\\V_1=5.00L\\M_2=12.39M\\V_2=?L

Putting values in above equation, we get:

6\times 5=12.39\times V_2\\\\V_2=2.42L

Hence, the volume of commercial HCl solution needed is 2.42 L.

5 0
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