Mole concept and stoichiometry Quiz 25 Q

Mole Concept & Stoichiometry Quiz

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Test your knowledge on mole concept and stoichiometry for JEE and NEET.

1. The number of moles in 46 g of sodium is:

• 1 mol
• 2 mol
• 0.5 mol
• 4 mol

2. What is the mass of 0.5 moles of $H_2SO_4$?

• 98 g
• 49 g
• 24.5 g
• 196 g

3. The number of atoms in 0.1 mol of a triatomic gas is:

• $6.022 \times 10^{22}$
• $1.806 \times 10^{23}$
• $3.011 \times 10^{23}$
• $6.022 \times 10^{23}$

4. What is the empirical formula of a compound that contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen by mass?

• $C_2H_4O_2$
• $CH_2O$
• $C_3H_6O_3$
• $C_6H_{12}O_6$

5. The volume occupied by 1 mole of a gas at STP is:

• 1 L
• 22.4 L
• 10 L
• 12.2 L

6. The limiting reagent in a chemical reaction is the reactant that:

• Is present in the largest amount.
• Is completely consumed in the reaction.
• Is left over after the reaction.
• Determines the rate of the reaction.

7. How many grams of $CO_2$ are produced from the complete combustion of 12 g of carbon?

• 44 g
• 22 g
• 12 g
• 33 g

8. What is the number of atoms in 4 g of He?

• $6.022 \times 10^{23}$
• $3.011 \times 10^{23}$
• $1.2044 \times 10^{24}$
• $6.022 \times 10^{24}$

9. The number of molecules in 16 g of methane ($CH_4$) is:

• $6.022 \times 10^{23}$
• $3.011 \times 10^{23}$
• $1.2044 \times 10^{24}$
• $6.022 \times 10^{24}$

10. What is the mass of one molecule of $H_2O$?

• 18 amu
• 18 g
• 1.8 g
• 18 kg

11. A sample of $CaCO_3$ has a mass of 50 g. What is the number of moles of calcium atoms in the sample?

• 1 mol
• 0.5 mol
• 2 mol
• 0.25 mol

12. The percentage composition of oxygen in $H_2SO_4$ is approximately:

• 32.65%
• 65.3%
• 16.3%
• 49%

13. The number of moles of water in 18 mL of water at room temperature is:

• 1 mol
• 0.5 mol
• 2 mol
• 1.5 mol

14. What is the molarity of a solution containing 4 g of NaOH in 250 mL of solution?

• 0.1 M
• 0.4 M
• 1.0 M
• 0.5 M

15. The number of electrons in 1 mole of methane ($CH_4$) is:

• $1.0 \times 10^{24}$
• $6.022 \times 10^{24}$
• $6.022 \times 10^{23}$
• $10 \times 6.022 \times 10^{23}$

16. The mass of 1 molecule of $CO_2$ is:

• 44 g
• 44 amu
• 44 kg
• $44 / (6.022 \times 10^{23})~g$

17. What is the number of moles of $O_2$ required to react completely with 4 moles of $C_2H_6$?

• 4 moles
• 7 moles
• 14 moles
• 12 moles

18. The number of hydrogen atoms in 18 g of water is:

• $6.022 \times 10^{23}$
• $1.2044 \times 10^{24}$
• $3.011 \times 10^{23}$
• $18 \times 6.022 \times 10^{23}$

19. A solution is prepared by dissolving 2 g of NaOH in water to make a 100 mL solution. What is the molarity of the solution?

• 0.5 M
• 1.0 M
• 2.0 M
• 0.2 M

20. What is the percentage of nitrogen in ammonia ($NH_3$)?

• 82.35%
• 17.65%
• 50%
• 75%

21. The number of moles of $H_2$ required to produce 10 moles of $NH_3$ is:

• 15 moles
• 10 moles
• 5 moles
• 20 moles

22. What is the number of moles of $NaCl$ in 100 mL of 0.5 M solution?

• 0.5 mol
• 0.05 mol
• 5 mol
• 0.005 mol

23. The number of moles of atoms in 34 g of $NH_3$ is:

• 2 mol
• 4 mol
• 8 mol
• 16 mol

24. What is the empirical formula of a compound with a molecular formula of $C_6H_{12}O_6$?

• $CH_2O$
• $C_2H_4O_2$
• $C_6H_{12}O_6$
• $C_3H_6O_3$

25. What is the mass of 1 mole of protons?

• 1 g
• 1 amu
• $6.022 \times 10^{23} \text{g}$
• $1.67 \times 10^{-24} \text{g}$

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