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A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas?
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A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its...
Explanation:
To find the empirical and molecular formulas of the compound, we need to follow the following steps:
Step 1: Find the empirical formula
The empirical formula of a compound shows the simplest whole number ratio of atoms present in the compound. To find the empirical formula, we need to assume that we have 100 grams of the compound. Then, we can calculate the number of moles of each element present in the compound using their percentage composition.
Given,
Hydrogen = 4.07%
Carbon = 24.27%
Chlorine = 71.65%
Let us assume that we have 100 grams of the compound.
Then, the mass of each element present in the compound would be:
Hydrogen = 4.07 grams
Carbon = 24.27 grams
Chlorine = 71.65 grams
Now, we can calculate the number of moles of each element using their molar masses:
Molar mass of hydrogen = 1.01 g/mol
Number of moles of hydrogen = 4.07/1.01 = 4.03
Molar mass of carbon = 12.01 g/mol
Number of moles of carbon = 24.27/12.01 = 2.02
Molar mass of chlorine = 35.45 g/mol
Number of moles of chlorine = 71.65/35.45 = 2.02
Next, we need to find the simple whole number ratio of atoms by dividing each of the above values by the smallest one. Here, the smallest value is 2.02.
Number of moles of hydrogen = 4.03/2.02 = 2
Number of moles of carbon = 2.02/2.02 = 1
Number of moles of chlorine = 2.02/2.02 = 1
Therefore, the empirical formula of the compound is H2CCl.
Step 2: Find the molecular formula
The molecular formula of a compound shows the actual number of atoms of each element present in a molecule of the compound. To find the molecular formula, we need to know the molar mass of the compound and the empirical formula.
Given,
Molar mass of the compound = 98.96 g/mol
Empirical formula of the compound = H2CCL
The empirical formula mass of the compound can be calculated as follows:
Empirical formula mass = (2 x molar mass of hydrogen) + (1 x molar mass of carbon) + (1 x molar mass of chlorine)
Empirical formula mass = (2 x 1.01 g/mol) + (1 x 12.01 g/mol) + (1 x 35.45 g/mol)
Empirical formula mass = 50.94 g/mol
Now, we can calculate the molecular formula of the compound by dividing the molar mass of the compound by the empirical formula mass:
Molecular formula mass = 98.96 g/mol
Dividing molecular mass by empirical mass = 98.96 g/mol / 50.94 g/mol = 1.94
Therefore, the molecular formula of the compound is (1.94) x (H2CCL) = H3.88C1.94Cl1.94.
However, we need to simplify this formula by
To find the empirical and molecular formulas of the compound, we need to follow the following steps:
Step 1: Find the empirical formula
The empirical formula of a compound shows the simplest whole number ratio of atoms present in the compound. To find the empirical formula, we need to assume that we have 100 grams of the compound. Then, we can calculate the number of moles of each element present in the compound using their percentage composition.
Given,
Hydrogen = 4.07%
Carbon = 24.27%
Chlorine = 71.65%
Let us assume that we have 100 grams of the compound.
Then, the mass of each element present in the compound would be:
Hydrogen = 4.07 grams
Carbon = 24.27 grams
Chlorine = 71.65 grams
Now, we can calculate the number of moles of each element using their molar masses:
Molar mass of hydrogen = 1.01 g/mol
Number of moles of hydrogen = 4.07/1.01 = 4.03
Molar mass of carbon = 12.01 g/mol
Number of moles of carbon = 24.27/12.01 = 2.02
Molar mass of chlorine = 35.45 g/mol
Number of moles of chlorine = 71.65/35.45 = 2.02
Next, we need to find the simple whole number ratio of atoms by dividing each of the above values by the smallest one. Here, the smallest value is 2.02.
Number of moles of hydrogen = 4.03/2.02 = 2
Number of moles of carbon = 2.02/2.02 = 1
Number of moles of chlorine = 2.02/2.02 = 1
Therefore, the empirical formula of the compound is H2CCl.
Step 2: Find the molecular formula
The molecular formula of a compound shows the actual number of atoms of each element present in a molecule of the compound. To find the molecular formula, we need to know the molar mass of the compound and the empirical formula.
Given,
Molar mass of the compound = 98.96 g/mol
Empirical formula of the compound = H2CCL
The empirical formula mass of the compound can be calculated as follows:
Empirical formula mass = (2 x molar mass of hydrogen) + (1 x molar mass of carbon) + (1 x molar mass of chlorine)
Empirical formula mass = (2 x 1.01 g/mol) + (1 x 12.01 g/mol) + (1 x 35.45 g/mol)
Empirical formula mass = 50.94 g/mol
Now, we can calculate the molecular formula of the compound by dividing the molar mass of the compound by the empirical formula mass:
Molecular formula mass = 98.96 g/mol
Dividing molecular mass by empirical mass = 98.96 g/mol / 50.94 g/mol = 1.94
Therefore, the molecular formula of the compound is (1.94) x (H2CCL) = H3.88C1.94Cl1.94.
However, we need to simplify this formula by
Community Answer
A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its...
1.03
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A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas?
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A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas?.
A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound contains 4.07% hydrogen 24. 27% carbon 71.65% chlorine, its molar mass is 98.96 gram. What are its empirical and molecular formulas?.
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