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Free_Kalibri [48]
3 years ago
7

What is the mass in grams of 9.76 × 1012 atoms of naturally occurring beryllium?

Chemistry
2 answers:
Ksivusya [100]3 years ago
8 0

The atomic mass of beryllium (Be) is 9 g/mole

Now, 1 mole of any substance contains avogadro's number of that substance. Therefore:

1 mole of Be contains 6.023  10^23 atoms of Be

In other words:

9 grams of Be contains 6.023*10^23 atoms of Be

Therefore, the mass corresponding to 9.76 * 10^12 atoms of Be is:

= 9 g * 9.76 10^12 atoms/6.023*10^23 atoms

= 1.458 * 10^-10 g (or) 1.46 * 10^-10 g


Reika [66]3 years ago
6 0

<u>Answer:</u> The mass of given number of atoms of beryllium is 1.46\times 10^{-10}g

<u>Explanation:</u>

Beryllium is the 4th element of the periodic table.

We know that:

Molar mass of beryllium = 9 g/mol

We are given:

Number of beryllium atoms = 9.76\times 10^{12}

According to mole concept:

6.022\times 10^{23} number of molecules occupy 1 mole of a gas.

As, 6.022\times 10^{23} number of beryllium atoms has a mass of 9 grams.

So, 9.76\times 10^{12} atoms of beryllium will have a mass of = \frac{9g}{6.022\times 10^{23}}\times 9.76\times 10^{12}=1.46\times 10^{-10}g

Hence, the mass of given number of atoms of beryllium is 1.46\times 10^{-10}g

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Given that:

Element A has 3 valence electrons and element B has 2 valence electrons. To find the ionic compound, the valency of the cations and the anions are interchanged and are written in subscripts. Thus,

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<u>Hence, 3 is the subscript for Element B.</u>

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Jaiden is writing a report about the structure of the atom. In her report, she says that the atom has three main parts and two s
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Sample Response: The change in her position (from beginning to end), along with the direction, is considered her displacement. T
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2 years ago
Select the true statements regarding these resonance structures of formate.? Each carbon-oyxgen bond is somewhere between a sing
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Again, the O atom with two bonds and two lone pairs on the resonance form left, changed into O atom with one bond and three lone pairs. It concludes that each carbon-oxygen bond is neither a single bond nor a double bond; each carbon-oxygen bond is somewhere between a single and double bond.

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7 0
3 years ago
Read 2 more answers
A standard solution of FeSCN2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO3)3 with 1.0 mL of 0.0020 M KSCN . The standard so
Xelga [282]

Answer : The equilibrium concentration of SCN^- in the trial solution is 4.58\times 10^{-8}M

Explanation :

First we have to calculate the initial moles of Fe^{3+} and SCN^-.

\text{Moles of }Fe^{3+}=\text{Concentration of }Fe^{3+}\times \text{Volume of solution}

\text{Moles of }Fe^{3+}=0.20M\times 9.0mL=1.8mmol

and,

\text{Moles of }SCN^-=\text{Concentration of }SCN^-\times \text{Volume of solution}

\text{Moles of }SCN^-=0.0020M\times 1.0mL=0.0020mmol

The given balanced chemical reaction is,

Fe^{3+}(aq)+SCN^-(aq)\rightleftharpoons FeSCN^{2+}(aq)

Since 1 mole of Fe^{3+} reacts with 1 mole of SCN^- to give 1 mole of FeSCN^{2+}

The limiting reagent is, SCN^-

So, the number of moles of FeSCN^{2+} = 0.0020 mmole

Now we have to calculate the concentration of FeSCN^{2+}.

\text{Concentration of }FeSCN^{2+}=\frac{0.0020mmol}{9.0mL+1.0mL}=0.00020M

Using Beer-Lambert's law :

A=\epsilon \times C\times l

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A = absorbance of solution

C = concentration of solution

l = path length

\epsilon = molar absorptivity coefficient

\epsilon and l are same for stock solution and dilute solution. So,

\epsilon l=\frac{A}{C}=\frac{0.480}{0.00020M}=2400M^{-1}

For trial solution:

The equilibrium concentration of SCN^- is,

[SCN^-]_{eqm}=[SCN^-]_{initial}-[FeSCN^{2+}]

[SCN^-]_{initial} = 0.00050 M

Now calculate the [FeSCN^{2+}].

C=\frac{A}{\epsilon l}=\frac{0.220}{2400M^{-1}}=9.17\times 10^{-5}M

Now calculate the concentration of SCN^-.

[SCN^-]_{eqm}=[SCN^-]_{initial}-[FeSCN^{2+}]

[SCN^-]_{eqm}=(0.00050M)-(9.17\times 10^{-5}M)

[SCN^-]_{eqm}=4.58\times 10^{-8}M

Therefore, the equilibrium concentration of SCN^- in the trial solution is 4.58\times 10^{-8}M

5 0
3 years ago
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