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4 years ago

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A certain compound is made up of one phosphorus (p) atom, three chlorine (cl) atoms, and one oxygen (o) atom. what is the chemic

al formula of this compound? note: you will need the periodic table for this question. express your answer as a chemical formula.

1 answer:

nikklg [1K]4 years ago

8 0

Phosphoryl chloride, O=PCL3

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The sample of oxygen gas was collected through water displacement. So, the gas collected will be a mixture of oxygen and water vapor.

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A 3.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of

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Answer: The molecular formula for the given organic compound X is $C_6H_{8}O_7$

Explanation:

We are given:

Mass of $CO_2=4.13g$

Mass of $H_2O=1.13g$

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 4.13 g of carbon dioxide, = $\frac{12}{44}\times 4.13=1.13g$ of carbon will be contained.

For calculating the mass of hydrogen:

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

So, in 1.13 g of water, $\frac{2}{18}\times 1.13=0.125g$ of hydrogen will be contained.

Mass of oxygen in the compound = (3.00) - (1.13+ 0.125) = 1.75 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.13g}{12g/mole}=0.094moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.125g}{1g/mole}=0.125moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.75g}{16g/mole}=0.109moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles

For Carbon = $\frac{0.094}{0.094}=1$

For Hydrogen = $\frac{0.125}{0.094}=1.33$

For Oxygen = $\frac{0.109}{0.094}=1.16$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 1: 1.33: 1.16

Converting them into whole number ratios by multiplying by 6:

The ratio of C : H : O = 6: 8: 7

Hence, the empirical formula for the given compound is $C_6H_8O_7$

Empirical mass = $6\times 12+8\times 1+7\times 16=192g$

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

Putting values in above equation, we get:

$n=\frac{192g/mol}{192g/mol}=1$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_6H_8O_7\times 1=C_6H_{8}O_7$

Thus molecular formula for the given organic compound X is $C_6H_{8}O_7$

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