Stoichiometry

Relative Atomic Mass is defined as the average mass of the atoms of an element compared to:

Calculate the relative molecular mass ($M_r$) of sulfuric acid, $H_2SO_4$. (Given $A_r$: $H=1, S=32, O=16$)

What is the relative molecular mass ($M_r$) of sulfur hexafluoride, $SF_6$? (Given $A_r$: $S=32, F=19$)

How many moles are in 2.2 g of Carbon Dioxide? (Relative formula mass: $CO_{2} = 44$)

What is the mass of 0.25 moles of Magnesium? (Relative atomic mass: $Mg = 24$)

Which formula relates moles, concentration, and volume of a solution?

A compound has an empirical formula of $CH_{2}$. Its molecular mass is 28. What is its molecular formula? ($A_{r}: C=12, H=1$)

If the molecular formula is $C_{10}H_{22}$, what is the empirical formula?

What is the empirical formula of a compound with $52.2\%$ C, $13.0\%$ H, and $34.8\%$ O? ($A_{r}: C=12, H=1, O=16$)

What is the volume of $4.8\,g$ of methane gas ($CH_4$) at RTP? ($M_r$ of $CH_4 = 16$, Molar volume = $24.0\,dm^3/mol$)

Calculate the mass of $1.5\,mol$ of carbon atoms, $C$. (Relative atomic mass: $C = 12$)

What is the relative formula mass of potassium chloride, $KCl$? (Relative atomic masses: $K = 39, Cl = 35.5$)