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Mdcat-past-papers - UHS Quiz

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



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



103. The atomic masses of element depend upon:



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



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



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



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



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



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



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



111. 8 g (4 moles) of H₂ react with 2 moles of O₂. How many moles of water are formed?



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



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



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



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



116. 3.0 moles of calcium will contain ----g of calcium:



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



118. The number of moles of water in 1kg of ice is:



119. How many moles of calcium carbonate are present in 77.5 kg of calcium carbonate? (Atomic mass of Ca = 40, C = 12, O = 16 → CaCO₃ = 100 g/mol)



120. 30 grams of 2-propanol were mixed with access acidified K2Cr2O7 and boiled under reflux for 20 min the organic product was than collected by distillation and 75% yield was obtained. What is the mass of product produced?



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