Mole Concept in Chemistry Quiz

Test your knowledge of stoichiometry with these questions on Avogadro's number, molar mass, gas laws, and more.

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1. What is the Avogadro's number?

6.022 x 10^23

3.142 x 10^8

9.81 x 10^5

2.997 x 10^10

2. How many moles of atoms are present in one mole of methane (CH4)?

6.022 x 10^23

8.022 x 10^23

8. What is the relationship between the mole and Avogadro's number?

1 mole = Avogadro's number

1 mole = 2 Avogadro's numbers

1 mole = 0.5 Avogadro's numbers

1 mole = 10 Avogadro's numbers

15. What is the molar volume of an ideal gas at standard temperature and pressure (STP)?

22.4 L/mol

24.0 L/mol

26.2 L/mol

28.5 L/mol

17. What is the relationship between the mass, moles, and molar mass of a substance?

Mass = Moles x Molar mass

MoLar mass = Mass / Moles

Moles = Mass / Molar mass

Mass = Moles / Molar mass

3. What is the molar mass of water (H2O)?

18 g/mol

22 g/mol

16 g/mol

10 g/mol

4. If 2 moles of a substance weigh 36 grams, what is its molar mass?

16 g/mol

18 g/mol

20 g/mol

22 g/mol

6. How many moles of oxygen (O2) molecules are there in 2 moles of ozone (O3)?

2 moles

3 moles

4 moles

6 moles

9. In a chemical reaction, if the reactants are in stoichiometric proportions, what is the relationship between their mole ratios?

Equal

Different

Dependent on temperature

Dependent on pressure

#10

11. If 18 grams of water (H2O) is present, how many moles of water molecules are there?

1 mole

2 moles

3 moles

4 moles

#11

5. What is the concept of the limiting reactant in a chemical reaction?

The reactant that limits the speed of the reaction

The reactant in excess quantity

The reactant that is completely consumed

The reactant that does not participate in the reaction

#12

7. If the empirical formula of a compound is CH2 and its molar mass is 42 g/mol, what is its molecular formula?

C2H4

C3H6

C4H8

C5H10

#13

10. What is the molarity of a solution containing 0.5 moles of solute in 250 mL of solution?

0.2 M

0.5 M

1.0 M

2.0 M

#14

12. What is the formula for percent composition?

(Mass of element / Molar mass of compound) x 100

(Molar mass of compound / Mass of element) x 100

(Number of moles of element / Total moles of compound) x 100

(Total moles of compound / Number of moles of element) x 100

#15

14. Which gas law is represented by the equation PV = nRT?

Boyle's Law

Charles's Law

Avogadro's Law

Ideal Gas Law