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3 years ago

How many grams of strontium (Sr, 87.62 g/mol) are in 2.92 moles of strontium?

Chemistry

2 answers:

S_A_V [24]3 years ago

8 0

Answer :The correct answer for mass of Sr is 255.85 g.

Mole :

It can defined as the amount of substance that contains as many entities as present 12 g of Carbon-12 .

In 1 mole of any atom , molecule or ions is equal to its atomic mass , molecular mass or ionic mass respectively .

Mass , molar mass ( or atomic mass or ionic mass ) and mole can be related as :

$Mole(mol) = \frac{ given mass (g)}{molar mass (\frac{g}{mol})}$

Given :

Molar mass of Strontium = 87.62 $\frac{g}{mol}$

Mole of Strontium = 2.92 mol

Plugging these values in Mole formula :

$2.92 mol = \frac{mass of Sr }{87.62 \frac{g}{mol}}$

Multiplying both side by 87.62 $\frac{g}{mol}$

$2.92 mol * 87.62 \frac{g}{mol}= \frac{mass of Sr }{87.62 \frac{g}{mol}} * 87.62 \frac{g}{mol}$

Mass of Sr = 255.85 g

kherson [118]3 years ago

3 0

Mass= number of mole *Molar mass
mass =2.92 mol*87.62 g/mol≈256 g

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3 years ago

A 0.1153-gram sample of a pure hydrocarbon was burned in a C-H combustion train to produce 0.3986 gram of CO2and 0.0578 gram of

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Answer: The mass of carbon and hydrogen in the sample is 0.1087 g and 0.0066 g respectively and the percentage composition of carbon and hydrogen in the sample is 94.27 % and 5.72 % respectively.

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The chemical equation for the combustion of hydrocarbon having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of $CO_2=0.3986g$

Mass of $H_2O=0.0578g$

Mass of sample = 0.1153 g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 0.3986 g of carbon dioxide, $\frac{12}{44}\times 0.3986=0.1087g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 0.0578 g of water, $\frac{2}{18}\times 0.0578=0.0066g$ of hydrogen will be contained.

To calculate the percentage composition of a substance in sample, we use the equation:

$\%\text{ composition of substance}=\frac{\text{Mass of substance}}{\text{Mass of sample}}\times 100$ ......(1)

For Carbon:

Mass of sample = 0.1153 g

Mass of carbon = 0.1087 g

Putting values in equation 1, we get:

$\%\text{ composition of carbon}=\frac{0.1087g}{0.1153g}\times 100=94.27\%$

For Hydrogen:

Mass of sample = 0.1153 g

Mass of hydrogen = 0.0066 g

Putting values in equation 1, we get:

$\%\text{ composition of hydrogen}=\frac{0.0066g}{0.1153g}\times 100=5.72\%$

Hence, the mass of carbon and hydrogen in the sample is 0.1087 g and 0.0066 g respectively and the percentage composition of carbon and hydrogen in the sample is 94.27 % and 5.72 % respectively.

8 0

3 years ago