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3 years ago

How many particles would be found in a 89.2 g sample of Na?

1 answer:

5 0

One mole of a substance contains 6.02 × 10∧23 particles. Thus we first convert 89.2 g to moles. 1 mole of sodium contains 23 g
Hence 89.2 g = 89.2 / 23 g = 3.878 moles
Therefore, 3.878 × 6.02×10∧23 particles= 23.346 × 10∧23 particles
Hence 89.2 g of sodium contains 2.335 ×10∧24 particles

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BigorU [14]

Answer:

Samarium

Explanation:

The element Sm describe is called Samarium. This element has unique sets of properties that makes it very unique and distinct.

The lanthanides are found in the f-block on the periodic table of elements.

This element is a moderately hard silvery metal that readily oxidizes in air. It assumes an oxidation state of +3. The element has an atomic number of 62

7 0

3 years ago

Circulacion de electrones en un material conductor en determinado tiempo.

barxatty [35]

Answer:

falso

Explanation:

tiempo no determinado El circulation de elctrones

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2 years ago

Electromagnetic energy released during fusion is converted to other kinds of photons as it is transferred through which layer of

Yuri [45]

Electromagnetic energy released during fusion is converted to other kinds of photons as it is transferred through the RADIATIVE layer of the sun. The sun is divided into five distinct layers, which are: the core, the radiative zone, the convective zone, the photosphere and the chromosphere.

3 0

3 years ago

Read 2 more answers

A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an

inysia [295]

<u>Answer:</u> The molar mass of the unknown compound is 223.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

where,

$\pi$ = osmotic pressure of the solution = 8.44 torr

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = $62.3637\text{ L torr }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$8.44torr=1\times M\times 62.3637\text{ L. torr }mol^{-1}K^{-1}\times 298K\\\\M=\frac{8.44}{1\times 62.3637\times 298}=4.54\times 10^{-4}M$

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

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

We are given:

Molarity of solution = $4.54\times 10^{-4}M$

Given mass of unknown compound = 15.2 mg = 0.0152 g (Conversion factor: 1 g = 1000 mg)

Volume of solution = 150.0 mL

Putting values in above equation, we get:

$4.54\times 10^{-4}M=\frac{0.0152\times 1000}{\text{Molar mass of unknown compound}\times 150.0}\\\\\text{Molar mass of unknown compound}=\frac{0.0152\times 1000}{150.0\times 4.54\times 10^{-4}}=223.2g/mol$

Hence, the molar mass of the unknown compound is 223.2 g/mol

5 0

3 years ago

When aluminum, Al, metal is dipped in an aqueous solution of hydrochloric acid, HCl, hydrogen gas, H2, is produced with the form

Alex17521 [72]

Answer:

2Al (s) + 6HCl (aq) → 2 AlCl3 (aq) + 3H2 (g)↑

Explanation:

- We can put an up arrow to H2 cause as it is a gas, it can be released to the atmosphere.

- Aluminum as metal must be solid.

- As we have two solutions, both are aqueous phase.

- The stoichiometry must match on both sides of the reaction to have the same amount of elements of each compound.}

Reactants : 2 Aluminun

6 Hydrogen

6 Chloride

Products:

2 Aluminun

2.3 = 6 Chloride

3.2 = 6 Hydrogen

8 0

3 years ago