Use of amount of substance in relation to masses of pure substances：練習題

Calculate the number of moles in \(25\text{g}\) of calcium carbonate, \(\text{CaCO}_{3}\).
(Relative atomic masses: \(\text{Ca} = 40\), \(\text{C} = 12\), \(\text{O} = 16\))

How many moles of substance are present in \(22\text{g}\) of carbon dioxide, \(\text{CO}_2\)?
(Relative atomic masses: \(\text{C} = 12\), \(\text{O} = 16\))

Define the term limiting reactant and explain its effect on the maximum amount of product that can be formed in a chemical reaction.

Calculate the mass in grams of \(0.25\) moles of sulfuric acid, \(\text{H}_2\text{SO}_4\).
(Relative atomic masses: \(\text{H} = 1\), \(\text{S} = 32\), \(\text{O} = 16\))

Calculate the theoretical mass of iron(III) oxide (\(Fe_{2}O_{3}\)) produced when 11.2 g of iron reacts completely with excess oxygen.
\(4Fe(s) + 3O_{2}(g) \rightarrow 2Fe_{2}O_{3}(s)\)
(Relative atomic masses: \(Fe = 56, O = 16\))

A student reacts 2.70 g of aluminum with an excess of copper(II) sulfate solution. The equation for the reaction is:
\(2Al(s) + 3CuSO_4(aq) \rightarrow Al_2(SO_4)_3(aq) + 3Cu(s)\)

Calculate the mass of copper produced in this reaction. Show all your working.

(Relative atomic masses: \(Al = 27, Cu = 63.5, S = 32, O = 16\))

Calculate the mass of iron(III) oxide (\(Fe_2O_3\)) that contains 11.2 g of iron atoms.

(Relative atomic masses: \(Fe = 56, O = 16\))