This set contains 50 MCQs focusing on mole calculations, conversion between mass and number of particles, molar mass applications, and numerical problems based on the mole concept. The questions test the ability to apply formulas for calculating moles, number of atoms/molecules, and mass of substances. These are essential for developing problem-solving skills in chemistry.
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📘 SCIENCE
CHEMISTRY | Atoms & Molecules-F
📝 Questions: 50
⏱️ Timer: 20 min
Q1. 18 u of water contains:
Q2. 18 g of water contains:
Q3. One mole of water contains:
Q4. Chemists need the number of atoms and molecules mainly for:
Q5. The relation between mass and number of particles is done using the:
Q6. One mole is equal to:
Q7. A mole is called the chemist's:
Q8. The word "mole" was introduced around the year:
Q9. The word "mole" was introduced by:
Q10. The word "mole" is derived from the Latin word:
Q11. The Latin word "moles" means:
Q12. The unit mole was officially accepted in the year:
Q13. One mole of any substance contains:
Q14. The Avogadro number is:
Q15. The atomic mass of helium (He) is:
Q16. The molar mass of helium is:
Q17. Number of moles is calculated using the formula:
Q18. The number of moles in 52 g of He is:
Q19. The symbol used for number of moles is:
Q20. The number of moles can also be calculated using:
Q21. Number of moles from particles is given by:
Q22. 12.044 × 10²³ He atoms are equal to:
Q23. The molar mass of nitrogen molecule (N₂) is:
Q24. The mass of 0.5 mole of N₂ gas is:
Q25. The molar mass of nitrogen atom is:
Q26. The mass of 0.5 mole of nitrogen atoms is:
Q27. 3.011 × 10²³ nitrogen atoms represent:
Q28. The mass of 3.011 × 10²³ nitrogen atoms is:
Q29. 6.022 × 10²³ molecules of N₂ represent:
Q30. The mass of 6.022 × 10²³ N₂ molecules is:
Q31. The number of particles from mass is calculated using:
Q32. The atomic mass of sodium (Na) is:
Q33. 46 g of sodium contains how many atoms?
Q34. The molar mass of O₂ molecule is:
Q35. 8 g of O₂ molecules correspond to:
Q36. The number of molecules in 0.1 mole of carbon atoms is:
Q37. The number of particles is calculated by:
Q38. If one mole of carbon weighs 12 g, then one atom of carbon weighs:
Q39. The atomic mass of iron (Fe) is:
Q40. 100 g of sodium has:
Q41. A substance can be considered as a heap of:
Q42. The mass of substance depends on the number of:
Q43. Avogadro number is named after:
Q44. The relationship between mass, mole and number is shown by:
Q45. Mole helps in converting:
Q46. The SI unit of amount of substance is:
Q47. The symbol of Avogadro number is:
Q48. Mole provides a simple way to report:
Q49. The molar mass of nitrogen atom is:
Q50. The mole concept is mainly used in:
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