CHEMISTRY HIGH SCHOOL

What is the mass of 3.0 x 10^23 atoms of neon

Answers

Answer 1

Answer:

The mass of 3.0 x 10^23 atoms of neon would be 10.09 g

According to Avogadro;

1 mole of neon would have 6.022 x 10^23 atoms

3.0 x 10^23 atoms of neon would have:

3.0 x 10^23/6.022 x 10^23

= 0.5 moles

mass of 0.5 moles neon = mole x molar mass

= 0.5 x 20.18

= 10.09 g

More on Avogadro number can be found here: brainly.com/question/1445383?referrer=searchResults

Answer 2

Answer:

Answer: The mass of neon for the given number of atoms will be 9.8 g.

Explanation:

We are given:

Number of neon atoms = $3.0* 10^(23)$

According to the mole concept:

$6.022* 10^(23)$ number of atoms. are occupied in 1 mole of a substance.

So, $3.0* 10^(23)$ will be occupied in = $(1)/(6.022* 10^(23))* 3.0* 10^(23)=0.49moles$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Moles of Neon = 0.49 moles

Molar mass of neon = 20 g/mol

Putting values in above equation, we get:

$0.49mol=\frac{\text{Mass of neon}}{20g/mol}\n\n\text{Mass of neon}=9.8g$

Hence, the mass of neon for the given number of atoms will be 0.49g.

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Answers

The net ionic equation is

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Explanation

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from above molecular equation break all soluble electrolyte into ions

Ag⁺(aq) +NO₃⁻ (aq) + K⁺(aq) +Cl⁻(aq) → AgCl (s) + K⁺(aq) + No₃⁻(aq)

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Answers

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