Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr₂(aq) + H₂(g)
What mass of HBr (in g) do you need to dissolve a 2.80-g pure iron bar on a padlock? What mass of H₂ would the complete reaction of the iron bar produce?

Consider the balanced equation:

SiO₂(s) + 3 C(s) → SiC(s) + 2 CO(g)

Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.

Find the limiting reactant for each initial amount of reactants. 2 Na(s) + Br₂( g) → 2 NaBr(s) c. 1.5 mol Na, 2.1 mol Br₂

Balance the equation and calculate how many moles of O₂ form when each quantity of reactant completely reacts. N₂O₅( g) → NO₂(g) + O₂(g) a. 1.2 mol N₂O₅

Sulfuric acid dissolves aluminum metal according to the reaction:

2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂(g)

Suppose you want to dissolve an aluminum block with a mass of 11.3 g. What minimum mass of H₂SO₄ (in g) do you need? What mass of H₂ gas (in g) does the complete reaction of the aluminum block produce?

Balance the equation and calculate how many moles of N₂ form when each quantity of reactant completely reacts. N₂H₄(l) → NH₃(g) + N₂(g) c. 33.9 g N₂H₄