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Mdcat-past-papers - UHS - Chemistry Quiz

Filters: Board: UHS | Subject: Chemistry |
1. While finding the relative atomic mass, which of the following is used to compare the atomic mass of chlorine (35.5 amu)?



2. One a.m.u stands for:



3. Which element is used as standard to determine atomic mass of an element?



4. The average weight of atoms of an element compared to the weight of one atom of ----- is called atomic weight.



5. The type and relative amount of each isotope in an element can be found by:



6. The atomic masses of element depend upon:



7. No individual atom in sample of 1 mole of Neon has a mass of 20.18 a.m.u. Because it is:



8. An organic compound has empirical formula C₃H₃O. If the molar mass is 110.15 g/mol, the molecular formula is:



9. A polymer has empirical formula CH3 and molar mass 28,000 g/mol. molecular formula is:



10. The formula showing the simplest whole-number ratio of atoms in a compound is:



11. A sodium oxide compound has 74.2% Na and 25.8% O. The empirical formula is:



12. A phosphorous oxide has 43.6% oxygen. Its empirical formula is:



13. How many chlorine atoms are in 2 moles of Cl₂?



14. 8 g (4 moles) of H₂ react with 2 moles of O₂. How many moles of water are formed?



15. Hydrogen burns in chlorine to produce HCl. The ratio of masses of reactants in the chemical reaction is: H₂ + Cl₂ → 2HCl



16. The number of molecules in 9g of ice (H₂O) is:



17. How many moles of sodium are present in 0.1g of sodium?



18. The number of moles of CO₂ which contains 8.00g of oxygen is:



19. 3.0 moles of calcium will contain ----g of calcium:



20. During stoichiometric calculations, which of the following laws must be followed?



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