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2 years ago

3. In an atomic model, what particles are found inside the nucleus of an atom?

Chemistry

1 answer:

sukhopar [10]2 years ago

4 0

Answer:

Neurons and Protons

Explanation:

The Electrons are outside of the nucleus, also known as the Electron Cloud.

I hope this was what you were looking for, and as always, I am joyous to assist anyone at any time.

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What is the result of adding 2.5 × 10³ and 3.5 × 10²?

Elanso [62]

Answer:

Explanation:

It is correct please I hope it helps! :)

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2 years ago

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A pupil adds 5 cm of 12 mol.dm sulphuric acids to make a 250 cmº solution. Calculate the

klemol [59]

Answer:

0.500 mol/dm³

Explanation:

Using the formula below;

CaVa = CbVb

Where;

Ca = concentration of acid (mol/dm³)

Cb = concentration of base (mol/dm³)

Va = volume of acid (cm³)

Vb = volume of base (cm³)

In accordance to the information provided in this question is;

Va = 5cm³

Vb = 250 cm³

Ca = 12 mol/dm³

Cb = ?

Using CaVa = CbVb

12 × 5 = Cb × 250

60 = 120Cb

Cb = 60/120

Cb = 0.500 mol/dm³

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2 years ago

Can anyone help me with this moon TGA?

kherson [118]

Answer:

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Explanation:

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2 years ago

13. Fill in the following table

Mandarinka [93]

Answer:

Potassium Bromide = KBr

Nitrogen dioxide = NO₂

Lithium oxide = Li₂O

Explanation:

Potassium Bromide (KBr)

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2 years ago

The concentrated sulfuric acid we use in the laboratory is 98.0% sulfuric acid by weight. Calculate the molality and molarity of

timama [110]

Answer : The molarity and molality of the solution is, 18.29 mole/L and 499.59 mole/Kg respectively.

Solution : Given,

Density of solution = $1.83g/cm^3=1.83g/ml$

Molar mass of sulfuric acid (solute) = 98.079 g/mole

98.0 % sulfuric acid by mass means that 98.0 gram of sulfuric acid is present in 100 g of solution.

Mass of sulfuric acid (solute) = 98.0 g

Mass of solution = 100 g

Mass of solvent = Mass of solution - Mass of solute = 100 - 98.0 = 2 g

First we have to calculate the volume of solution.

$\text{Volume of solution}=\frac{\text{Mass of solution}}{\text{Density of solution}}=\frac{100g}{1.83g/ml}=54.64ml$

Now we have to calculate the molarity of solution.

$Molarity=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{volume of solution}}=\frac{98.0g\times 1000}{98.079g/mole\times 54.64ml}=18.29mole/L$

Now we have to calculate the molality of the solution.

$Molality=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Mass of solvent}}=\frac{98.0g\times 1000}{98.079g/mole\times 2g}=499.59mole/Kg$

Therefore, the molarity and molality of the solution is, 18.29 mole/L and 499.59 mole/Kg respectively.

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2 years ago