Relative Atomic Mass and Relative Molecular Mass
Chemistry ⇒ Atomic Structure and the Periodic Table
Relative Atomic Mass and Relative Molecular Mass starts at 9 and continues till grade 12.
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See sample questions for grade 11
A molecule of ammonia (NH3) contains 1 nitrogen atom and 3 hydrogen atoms. Calculate its relative molecular mass. (N = 14.0, H = 1.0)
A molecule of glucose (C6H12O6) contains 6 carbon, 12 hydrogen, and 6 oxygen atoms. Calculate its relative molecular mass. (C = 12.0, H = 1.0, O = 16.0)
A sample of boron contains 20% 10B (mass = 10) and 80% 11B (mass = 11). Calculate the relative atomic mass of boron.
A sample of chlorine contains 75% 35Cl (atomic mass = 35) and 25% 37Cl (atomic mass = 37). Calculate the relative atomic mass of chlorine.
A sample of element X contains 60% isotope X-29 (mass = 29) and 40% isotope X-30 (mass = 30). Calculate the relative atomic mass of X.
Calculate the relative formula mass of sodium sulfate (Na2SO4). (Na = 23.0, S = 32.1, O = 16.0)
Calculate the relative molecular mass of calcium carbonate (CaCO3). (Ca = 40.1, C = 12.0, O = 16.0)
Calculate the relative molecular mass of water (H2O). (Relative atomic masses: H = 1.0, O = 16.0)
Describe how the relative atomic mass of an element is determined experimentally.
Explain the difference between relative atomic mass and mass number.
Explain why the relative atomic mass of most elements is not a whole number.
Explain why the relative molecular mass of a compound is important in chemical calculations.
The relative atomic mass of magnesium is 24.3. What does this value represent?
What is meant by the term 'relative atomic mass'?
