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 10
A molecule of glucose has the formula C6H12O6. Calculate its relative molecular mass. (C = 12, H = 1, O = 16)
A sample contains 60% 63Cu (relative atomic mass = 63) and 40% 65Cu (relative atomic mass = 65). Calculate the relative atomic mass of copper.
A sample of chlorine contains 75% 35Cl (relative atomic mass = 35) and 25% 37Cl (relative atomic mass = 37). Calculate the relative atomic mass of chlorine.
Calculate the relative molecular mass (Mr) of water (H2O). (Relative atomic masses: H = 1, O = 16)
Calculate the relative molecular mass of calcium carbonate (CaCO3). (Ca = 40, C = 12, O = 16)
Calculate the relative molecular mass of ethane (C2H6). (C = 12, H = 1)
Describe the steps you would take to calculate the relative molecular mass of a compound given its chemical formula and the relative atomic masses of its elements.
Explain why the relative atomic mass of an element is important in chemistry.
Explain why the relative atomic mass of an element is not always 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'?
A compound has the empirical formula CH2O and a relative molecular mass of 180. What is its molecular formula? (C = 12, H = 1, O = 16)
A molecule of aluminium sulfate has the formula Al2(SO4)3. Calculate its relative molecular mass. (Al = 27, S = 32, O = 16)
A sample of bromine contains two isotopes: 50.7% 79Br (relative atomic mass = 78.918) and 49.3% 81Br (relative atomic mass = 80.916). Calculate the relative atomic mass of bromine to three decimal places.
A student claims that the relative molecular mass of a compound is always equal to the sum of the mass numbers of its atoms. Critically evaluate this statement.
Explain, with an example, how the presence of isotopes affects the calculation of the relative atomic mass of an element.
