Question

Methanol (methyl alcohol), \(\mathrm{CH}_{3} \mathrm{OH},\) is a very important industrial chemical. Formerly, methanol was prepared by heating wood to high temperatures in the absence of air. The complex compounds present in wood are degraded by this process into a charcoal residue and a volatile portion that is rich in methanol. Today, methanol is instead synthesized from carbon monoxide and elemental hydrogen. Write the balanced chemical equation for this latter process.

Short answer

The balanced chemical equation for the synthesis of methanol ($) \mathrm{CH}_{3} \mathrm{OH} $) from carbon monoxide (CO) and elemental hydrogen ($\mathrm{H}_{2}$) is: \[ \mathrm{CO} + 2\mathrm{H}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{OH} \]

Step-by-step solution

1. Write down the unbalanced chemical equation

First, write down the unbalanced equation using reactants and products given: \[ \mathrm{CO} + \mathrm{H}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{OH} \]

2. Count the atoms on each side of the equation

By counting the atoms of each type, we find that unbalanced equation has: - Reactants: 1 Carbon, 1 Oxygen, and 2 Hydrogen atoms - Products: 1 Carbon, 1 Oxygen, and 4 Hydrogen atoms

3. Balance the equation by adjusting the coefficients

To balance the hydrogen atoms, we need to multiply the H2 molecule by 2 as it is the only source of hydrogen atoms for the reaction. So we have: \[ \mathrm{CO} + 2\mathrm{H}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{OH} \]

4. Verify the balanced equation

We need to confirm that the balanced equation has the same number of atoms for each element on both sides. The balanced equation now has: - Reactants: 1 Carbon, 1 Oxygen, and 4 Hydrogen atoms - Products: 1 Carbon, 1 Oxygen, and 4 Hydrogen atoms The final balanced chemical equation for the synthesis of methanol from carbon monoxide and elemental hydrogen is: \[ \mathrm{CO} + 2\mathrm{H}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{OH} \]

Key concepts

Methanol Synthesis

Methanol synthesis is a fascinating process that has become essential in modern industrial practices. Methanol, often referred to as wood alcohol, was initially produced by a method known as destructive distillation of wood. However, due to advancements in chemical manufacturing, methanol is now synthesized via a more efficient method. This involves the chemical reaction between carbon monoxide (CO) and hydrogen gas (H₂).

This reaction takes place under high pressure and temperature conditions in the presence of a catalyst. The main reason for this method being preferred over traditional wood distillation is its efficiency and sustainability.

• The process creates fewer byproducts.
• It is a quicker method of production.
• More environmentally friendly as it uses carbon-based gases.

The synthesis of methanol is not only a testament to industrial innovation but also a cornerstone of modern chemical processes as it provides a renewable way to produce a vital chemical compound.

Chemical Reactions

Chemical reactions are processes through which substances, known as reactants, are transformed into different substances called products. In the case of methanol synthesis, the chemical reaction involves the transformation of carbon monoxide (CO) and hydrogen gas (H₂) into methanol (CH₃OH). The basic nature of chemical reactions can be categorized as either exothermic or endothermic based on whether they release or absorb heat.

The methanol synthesis reaction follows a simple formula expressed as:

• Reactants: CO + 2H₂
• Product: CH₃OH

For a chemical reaction to proceed, the reactants must collide with sufficient energy and proper orientation. This reaction is often catalyzed by metal catalysts, typically copper, which lowers the activation energy and speeds up the reaction.

Understanding chemical reactions is crucial in the study of chemistry. It helps in predicting how substances interact, whether the reactions will proceed, and what products will be formed.

Industrial Chemistry

Industrial chemistry plays a pivotal role in the scale-up and application of chemical reactions for manufacturing processes. The synthesis of methanol is a prime example where principles of industrial chemistry are applied. Utilizing catalysts and high-pressure reactors, the reaction between CO and H₂ shifts from the laboratory to large-scale production.

Key elements of industrial chemistry include:

• Optimization of reaction conditions to maximize yield.
• Cost efficiency through energy management.
• Environmental considerations and sustainability.

By focusing on these areas, the industrial production of methanol is made feasible and economically beneficial. This field extends into refining the production process, ensuring that reactions are not only efficient but also safe and environmentally sustainable. The integration of technology and chemistry in industrial settings enhances our ability to meet global chemical demands.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It plays a crucial role in methanol synthesis by determining the exact proportions of carbon monoxide and hydrogen required to produce methanol efficiently.

To balance a reaction like that of methanol synthesis, the stoichiometric coefficients must match the number of atoms of each element on both sides of the equation. For example, in the balanced equation:

• CO + 2H₂ → CH₃OH
• There is 1 carbon atom, 1 oxygen atom, and 4 hydrogen atoms on both sides.

This balance is achieved by modifying the coefficients in front of each reactant and product, ensuring that mass is conserved in the reaction.

Stoichiometry allows chemists to calculate necessary reactants for desired product quantities, optimizing resource use, and minimizing waste. Thus, this concept is a fundamental aspect of both laboratory research and industrial chemical production.