Question

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over a catalyst at \(800^{\circ} \mathrm{C}\). Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.

Short answer

(a) 2 CH₄ + 2 NH₃ + 3 O₂ → 2 HCN + 6 H₂O (b) NaHCO₃ + HCl → NaCl + CO₂ + H₂O (c) BaCO₃ + SO₂ → BaSO₄ + CO₂

Step-by-step solution

Reaction (a) reactants and products

First, let's identify the reactants and products for the formation of hydrogen cyanide. The reactants are methane (CH₄), ammonia (NH₃), and air (we can assume that oxygen (O₂) is the relevant component of air for this reaction). The products are hydrogen cyanide (HCN) and water (H₂O).

Balanced equation for reaction (a)

Now we write the balanced chemical equation for the formation of hydrogen cyanide: 2 CH₄ + 2 NH₃ + 3 O₂ → 2 HCN + 6 H₂O This equation is balanced as there are an equal number of atoms for each element on both sides of the equation.

Reaction (b) reactants and products

For the reaction of baking soda (NaHCO₃) with an acid (HCl, for example), the products are carbon dioxide (CO₂), water (H₂O), and a salt (NaCl).

Balanced equation for reaction (b)

Next, we write the balanced chemical equation for the reaction of baking soda with an acid: NaHCO₃ + HCl → NaCl + CO₂ + H₂O This equation is balanced as there are an equal number of atoms for each element on both sides of the equation.

Reaction (c) reactants and products

In the reaction of barium carbonate (BaCO₃) with sulfur dioxide (SO₂), the products are barium sulfate (BaSO₄) and carbon dioxide (CO₂).

Balanced equation for reaction (c)

Finally, we write the balanced chemical equation for the reaction of barium carbonate with sulfur dioxide: BaCO₃ + SO₂ → BaSO₄ + CO₂ This equation is balanced as there are an equal number of atoms for each element on both sides of the equation.