Chemistry Exam > Chemistry Questions > A compound has the empirical formula C10H8Fe....
Start Learning for Free
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?
- a)C30H24Fe3
- b)C10H8Fe
- c)C5H4Fe
- d)C20H16Fe2
Correct answer is option 'D'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of ...
Given data:
Empirical formula of the compound = C10H8Fe
Mass of the compound = 0.26 g
Mass of benzene = 11.2 g
Boiling point of benzene = 80.10C
Boiling point of solution = 80.26C
Kb of benzene = 2.53C/molal
To find: Molecular formula of the compound
Steps involved:
1. Calculate the molality of the solution
2. Calculate the change in boiling point of the solution
3. Calculate the number of moles of the compound in the solution
4. Calculate the molar mass of the compound
5. Find the molecular formula of the compound
1. Calculation of Molality:
Molality of the solution, m = (moles of solute) / (mass of solvent in kg)
Here, mass of solvent = 11.2 g = 0.0112 kg
Empirical formula weight of C10H8Fe = 160 g/mol
Moles of C10H8Fe in 0.26 g = 0.26 g / 160 g/mol = 0.001625 mol
Molality (m) = 0.001625 mol / 0.0112 kg = 0.145 mol/kg
2. Calculation of Change in Boiling Point (∆Tb):
∆Tb = Kb x m
Here, Kb = 2.53C/molal and m = 0.145 mol/kg
∆Tb = 2.53 C/molal x 0.145 mol/kg = 0.366 C
3. Calculation of Moles of the Compound:
∆Tb = Kb x m = (Kb x w2) / (Mf x Kb)
Here, w2 = mass of the compound = 0.26 g
Mf = molar mass of the compound
0.366 C = (2.53 C/molal x 0.26 g) / (Mf x 0.0112 kg)
Mf = 346.3 g/mol
Moles of the compound = 0.26 g / 346.3 g/mol = 0.000750 mol
4. Calculation of Molar Mass of the Compound:
Empirical formula weight of C10H8Fe = 160 g/mol
Molecular formula weight of the compound = 346.3 g/mol
Ratio of molecular formula weight to empirical formula weight = 346.3 g/mol / 160 g/mol = 2.165
The molecular formula of the compound should have a ratio of 2.165 times the empirical formula weight.
Therefore, the molecular formula of the compound = 2.165 x C10H8Fe = C20H16Fe2
Hence, the correct answer is option D, C20H16Fe2.
Empirical formula of the compound = C10H8Fe
Mass of the compound = 0.26 g
Mass of benzene = 11.2 g
Boiling point of benzene = 80.10C
Boiling point of solution = 80.26C
Kb of benzene = 2.53C/molal
To find: Molecular formula of the compound
Steps involved:
1. Calculate the molality of the solution
2. Calculate the change in boiling point of the solution
3. Calculate the number of moles of the compound in the solution
4. Calculate the molar mass of the compound
5. Find the molecular formula of the compound
1. Calculation of Molality:
Molality of the solution, m = (moles of solute) / (mass of solvent in kg)
Here, mass of solvent = 11.2 g = 0.0112 kg
Empirical formula weight of C10H8Fe = 160 g/mol
Moles of C10H8Fe in 0.26 g = 0.26 g / 160 g/mol = 0.001625 mol
Molality (m) = 0.001625 mol / 0.0112 kg = 0.145 mol/kg
2. Calculation of Change in Boiling Point (∆Tb):
∆Tb = Kb x m
Here, Kb = 2.53C/molal and m = 0.145 mol/kg
∆Tb = 2.53 C/molal x 0.145 mol/kg = 0.366 C
3. Calculation of Moles of the Compound:
∆Tb = Kb x m = (Kb x w2) / (Mf x Kb)
Here, w2 = mass of the compound = 0.26 g
Mf = molar mass of the compound
0.366 C = (2.53 C/molal x 0.26 g) / (Mf x 0.0112 kg)
Mf = 346.3 g/mol
Moles of the compound = 0.26 g / 346.3 g/mol = 0.000750 mol
4. Calculation of Molar Mass of the Compound:
Empirical formula weight of C10H8Fe = 160 g/mol
Molecular formula weight of the compound = 346.3 g/mol
Ratio of molecular formula weight to empirical formula weight = 346.3 g/mol / 160 g/mol = 2.165
The molecular formula of the compound should have a ratio of 2.165 times the empirical formula weight.
Therefore, the molecular formula of the compound = 2.165 x C10H8Fe = C20H16Fe2
Hence, the correct answer is option D, C20H16Fe2.
Free Test
FREE
| Start Free Test |
Community Answer
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of ...
|
Explore Courses for Chemistry exam
|
|
Similar Chemistry Doubts
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer?
Question Description
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer?.
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer?.
Solutions for A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
Download more important topics, notes, lectures and mock test series for Chemistry Exam by signing up for free.
Here you can find the meaning of A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer?, a detailed solution for A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A compound has the empirical formula C10H8Fe. A solution of 0.26 g of the compound in 11.2 g of benzene (C6H6) boils at 80.26°C. The boiling point of benzene is 80.10°C; the Kb is 2.53°C/molal. What is the molecular formula of the compound?a)C30H24Fe3b)C10H8Fec)C5H4Fed)C20H16Fe2Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice Chemistry tests.
|
|
Explore Courses for Chemistry exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup