This set of Class 11 Chemistry Chapter 1 Multiple Choice Questions & Answers (MCQs) focuses on “Percentage Composition”.
1. A _______ formula represents a whole number ratio to the simplest form.
a) Molecular
b) Empirical
c) Simpler
d) Shorter
View Answer
Explanation: An empirical formula is the simplest whole number ratio of various atoms present in a compound. The molecular formula is the exact number of different types of atoms present in the molecule of a compound.
2. Even without knowing the mass percent of each element, we can calculate the empirical formula.
a) True
b) False
View Answer
Explanation: One must know the mass percent of each and every element of a compound to calculate an empirical formula. As an empirical formula is the simplest whole number ratio of various atoms present in a compound.
3. __________ formula can be calculated if the molar mass is known after having an empirical formula.
a) Molecular
b) Empirical
c) Simpler
d) Shorter
View Answer
Explanation: The molecular formula is the exact number of different types of atoms present in the molecule of a compound. An empirical formula is the simplest whole number ratio of various atoms present in a compound. Therefore we can calculate the molecular formula if the molar mass is known.
4. Which of the following is an empirical formula?
a) C6H12O6
b) H2O2
c) CH4
d) C2H6
View Answer
Explanation: An empirical formula is the simplest whole number ratio of various atoms present in a compound. Only CH4 has satisfied the conditions of an empirical formula as it is the simplified whole number ratio compound.
5. The molecular formula of a compound is C6H12O6. What’s the empirical formula for this compound?
a) C6H12O6
b) CHO
c) C2H6O2
d) CH2O
View Answer
Explanation: In the molecular formula of glucose that is C6H12O6, the carbon, hydrogen, and oxygen are in the ratio of 6:12:6 respectively. So by simplifying them into simpler whole numbers, we obtain 1:2:1. Therefore the empirical formula is CH2O.
6. A compound consists of 52.17% of carbon, 13.04% of hydrogen and 34.78% of oxygen. Find the molecular formula if the given molecular weight of the compound is 46g.
a) C2H5OH
b) C2H6
c) C6H12O6
d) CH2O
View Answer
Explanation: As per the above question, the compounds consist of carbon, hydrogen, and oxygen in the ratio of 52.17:13.04:34.78 respectively. Now multiply the ratio with the molecular mass that is 46 g. Hence we obtain it as 2400:600:1600 that is 24:6:16 (2 atoms of carbon + 6 atom of hydrogen + 1 atom of oxygen). The required compound is C2H5OH.
7. Which of the following cannot be a molecular formula for an empirical formula HO?
a) H2O
b) H2O2
c) HO
d) HO2
View Answer
Explanation: The molecular formula is the exact number of different types of atoms present in the molecule of a compound. The rest compounds are not in the same ratio as of empirical formula ones. Though HO is possible, it can’t exist.
8. In glucose simplest ratio between C, H and O is ________
a) 6:12:6
b) 3:4:3
c) 1:2:1
d) 2:3:2
View Answer
Explanation: the molecular formula of glucose is C6H12O6. The ratio in the molecular formula is 6:12:6; carbon, hydrogen, and oxygen respectively. So by simplifying them into simpler whole numbers, we obtain 1:2:1.
9. Which of the following is true regarding molecular formula?
a) actual whole numbered ratio
b) rational numbered ratio
c) simplest possible whole numbered ratio
d) the same as the empirical ratio
View Answer
Explanation: Actual whole numbered ratio is correct because the molecular formula is the exact number of different types of atoms present in the molecule of a compound. Rational may be fractional or decimal, simplest possible whole numbered is empirical.
10. Which of the following cannot be an empirical formula?
a) NH3
b) C5H10
c) H2O
d) NaCl
View Answer
Explanation: C5H10 cannot be an empirical formula because of the carbon and hydrogen ratio in this compound is 5:10 respectively. They are not in the simplest possible whole numbered ratio (1:2 is the simplest for this compound). Hence it cannot be an empirical compound.
Sanfoundry Global Education & Learning Series – Chemistry – Class 11.
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