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2 years ago

What is the atomic number for an element with 6 neutrons and a mass number of 10

Chemistry

2 answers:

Rasek [7]2 years ago

6 0

Answer:

Thus,thenumberofprotonsis4

Whitepunk [10]2 years ago

5 0

$\bold{\huge{\blue{\underline{Answer}}}}$

$\bold{\underline{ Given :- }}$

Atomic number of an element with 6 neutrons and a mass number of 10

$\bold{\underline{ Let's \:Begin}}$

$\sf{We\: know\: that, }$

Atomic number is the number of protons in the nucleus of an atom

$\sf{Whereas ,}$

Mass number is the sum of protons and neutrons in the nucleus of an atom.

$\sf{We\: have \:number \:of \:neutrons = 6 }$

$\sf{ Mass\: number = 10 }$

$\bold{\underline{Therefore}}$

$\sf{ Mass\: number = Protons + neutrons}$

$\sf{ 10 = Protons + 6 }$

$\sf{ Protons = 10 - 6}$

$\sf{ Protons = 4 }$

$\sf{ Thus, \: the \: number \: of \: protons \: is \:4}$

$\bold{\underline{ Therefore,\:we\:know\:that, }}$

$\sf{ No\: of\: protons = Atomic \:number }$

$\sf{ 4 = Atomic \:number }$

$\sf { Hence, \:atomic\: number\: of\: the\: element\: is\: 4}$

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An element's ability to react with acid is an example of a

Dmitry [639]

Answer:

it's chemical property

Explanation:

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3 years ago

Analysis of a compound of sulfur, oxygen and fluorine showed that it is 31.42% S and 31.35% O, with F accounting for the remaind

Leya [2.2K]

Answer:

The molecular formula is SO2F2

Explanation:

Step 1: Data given

Suppose the mass of compound = 100 grams

The compound contains:

31.42 % S = 31.42 grams S

31.35 % O = 31.35 grams O

100 - 31.42 - 31.35 = 37.23 F

Molar mass of S = 32.065 g/mol

Molar mass F = 19.00 g/mol

Molar mass O = 16.00 g/mol

Step 2: Calculate moles

Moles = mass / molar mass

Moles S = 31.42 grams / 32.065 g/mol

Moles S = 0.9799 moles

Moles 0 = 31.35 grams / 16.00 g/mol

Moles 0 = 1.959 moles

Moles F = 37.23 grams / 19.00 g/mol

Moles F = 1.959 moles

Step 3: Calculate mol ratio

We divide by the smallest amount of moles

S: 0.9799 / 0.9799 = 1

F: 1.959/ 0.9799 = 2

O : 1.959 / 0.9799 = 2

The empirical formula is SO2F2

This formula has a molecular mass of 102.06 g/mol

This means the empirical formula is also the molecular formula : SO2F2

3 0

3 years ago

Find the density of metal with a volume 4.0 cm and a mass of 8.0 grams.

olga_2 [115]

D=m/v

so,

d=8.0g/4.0cm

d=2

3 0

3 years ago

The cell membrane is<br> a)semi permeable<br> b)selectively permeable

likoan [24]

Answer:

A. Semi Permeable.

Explanation:

Cell membranes are semi permeable.

7 0

2 years ago

A reaction of 41.9 g of Na and 30.3 g of Br2 yields 36.4 g of NaBr . What is the percent yield?

Licemer1 [7]

Answer: The percent yield is, 93.4%

Explanation:

First we have to calculate the moles of Na.

$\text{Moles of Na}=\frac{\text{Mass of Na}}{\text{Molar mass of Na}}=\frac{41.9g}{23g/mole}=1.82moles$

Now we have to calculate the moles of $Br_2$

${\text{Moles of}Br_2} = \frac{\text{Mass of }Br_2 }{\text{Molar mass of} Br_2} =\frac{30.3g}{160g/mole}=0.189moles$

${\text{Moles of } NaBr} = \frac{\text{Mass of } NaBr }{\text{Molar mass of } NaBr} =\frac{36.4g}{103g/mole}=0.353moles$

The balanced chemical reaction is,

$2Na(s)+Br_2(g)\rightarrow 2NaBr$

As, 1 mole of bromine react with = 2 moles of Sodium

So, 0.189 moles of bromine react with = $\frac{2}{1}\times 0.189=0.378$ moles of Sodium

Thus bromine is the limiting reagent as it limits the formation of product and Na is the excess reagent.

As, 1 mole of bromine give = 2 moles of Sodium bromide

So, 0.189 moles of bromine give = $\frac{2}{1}\times 0.189=0.378$ moles of Sodium bromide

Now we have to calculate the percent yield of reaction

$\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\times 100=\frac{0.353 mol}{0.378}\times 100=93.4\%$

Therefore, the percent yield is, 93.4%

3 0

3 years ago