Iron is obtained from iron(III) oxide. In the following series of reactions, (step 1) hot air (O₂) reacts with coke (C) to produce CO₂ and heat up the blast furnace, (step 2) additional coke reduces CO₂ into CO, and (step 3) the very high temperature allows for CO to reduce Fe in Fe₂O₃.

(Step 1) C (s) + O₂ (g) → CO₂ (g)
(Step 2) CO₂ (g) + C (s) → 2 CO (g)
(Step 3) Fe₂O₃ (s) + 3 CO (g) → 2 Fe (l) + 3 CO₂ (g)

Write mole ratios to show the relationship between reaction components.

The diagram below represents the reaction: X₂ + 3 Y₂ → 2 XY₃.

Determine the number of moles of product that can form from (i) 2.0 mol X₂ and (ii) 2.0 mol Y₂.

For the following unbalanced reaction: Na(s) + H₂SO₄(aq) → Na₂SO₄(aq) + H₂(g). Calculate the amount (in moles) of sodium sulfate produced from 8.00 mol Na and 14.0 mol of H₂SO₄.

The balanced reactions below shows the combustion of propane:

C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g) 

If 132.1 g of C₃H₈(g) is completely combusted, calculate the mass in grams of oxygen needed for this process.

Assuming that the reaction below goes to 100% completion, calculate the mass of each reactant needed to produce 360 L of water with a molar mass of 18.013 g/mol. The density of water is 1.00 g/mL.

2 H₂ (g) + O₂ (g) → 2 H₂O (l)

Consider the following reaction: 

3 NaBH₄ (aq) + 4 BF₃ (g)→ 3 NaBF₄ (aq) + 2 B₂H₆ (g)

Calculate the number of hydrogen atoms in the B₂H₆ produced if 16.5 moles of NaBF₄ are also formed.