Question

The compound which can consume 3 mole of per mole is (A) Ethylene glycol (B) Glycerol (C) Carbolic acid (D) Tertiary butanol

Short answer

Although none of the given compounds consume exactly 3 moles of oxygen per mole of compound, Glycerol (B) consumes the highest amount of oxygen (1 mole per mole of glycerol) and is the closest to the desired 3 moles of oxygen consumption.

Step-by-step solution

Write the molecular formulas for the given compounds

We need to write the molecular formula for each compound to better understand their structure and components. Here are the formulas for the compounds given in the problem: (A) Ethylene glycol: \(C_2H_6O_2\) (B) Glycerol: \(C_3H_8O_3\) (C) Carbolic acid (Phenol): \(C_6H_6O\) (D) Tertiary butanol: \(C_4H_{10}O\)

Determine the number of moles of consumed oxygen for each compound

Now we need to determine how many moles of oxygen would be consumed per mole of each compound. This can be done by observing the number of oxygen atoms in the molecular formula and considering how many moles of oxygen would be required to balance the chemical equation for complete combustion of these compounds. (A) Ethylene glycol: For every 1 mole of ethylene glycol, it requires 1.5 moles of oxygen for complete combustion. (B) Glycerol: For every 1 mole of glycerol, it requires 1 mole of oxygen for complete combustion. (C) Carbolic acid: For every 1 mole of carbolic acid, it requires approximately 0.5 moles of oxygen for complete combustion. (D) Tertiary butanol: For every 1 mole of tertiary butanol, it requires approximately 0.5 moles of oxygen for complete combustion.

Identify the compound that consumes 3 moles of oxygen

Now, we will compare the amount of moles of oxygen consumed by each compound to find the one that consumes 3 moles of oxygen per mole of the compound. From step 2, we can see that none of the given compounds consumes exactly 3 moles of oxygen per mole of compound. However, we can observe that Glycerol (B) consumes the highest amount of oxygen, which is 1 mole per mole of glycerol (closest to 3 moles of oxygen per mole of compound).

Conclusion

Based on our analysis, we can conclude that although none of the given compounds consume exactly 3 moles of oxygen per mole of compound, Glycerol (B) consumes the highest amount of oxygen (1 mole per mole of glycerol) and is the closest to the desired 3 moles of oxygen consumption.

Key concepts

Molecular Formula

Understanding the molecular formula of a compound is akin to having a recipe for a dish—it tells you exactly what and how much of each ingredient you need. In the context of organic chemistry, a molecular formula provides detailed information about the types and numbers of atoms in a molecule. For example, ethylene glycol has the molecular formula of \(C_2H_6O_2\). This tells us it contains two carbon atoms (C), six hydrogen atoms (H), and two oxygen atoms (O).

When we're examining combustion reactions or any chemical process, knowing the molecular formula is crucial since it allows us to predict and understand how compounds interact. It's the first step towards visualizing the molecules and preparing for the subsequent steps of balancing equations and performing stoichiometric calculations.

In the specific exercise, the molecular formula helped identify how much oxygen was needed per mole of a substance during combustion, which is vital for the next stages of problem-solving.

Chemical Reaction Balancing

The principle of conservation of mass dictates that the number of atoms of each element must remain the same before and after a chemical reaction. This is why we balance chemical reactions. For the given compounds, we would write chemical equations for their combustion and then balance them to ensure that the number of atoms for each element is equal on both sides of the equation.

For instance, the combustion of ethylene glycol can be represented as \( C_2H_6O_2 + O_2 \rightarrow CO_2 + H_2O \). However, to balance this reaction, coefficients must be placed before each molecule to ensure that the amount of each atom is conserved. Balancing requires careful attention and understanding of the molecular formulas and stoichiometry, to make calculated adjustments that reflect true chemical changes.

Stoichiometry

Stoichiometry is the aspect of chemistry that pertains to calculating the quantities of reactants and products in a chemical reaction. It's a mathematical approach to chemistry that allows chemists to make predictions about the outcomes of reactions. In the exercise provided, stoichiometry was essential to determine the consumption of oxygen during combustion. Knowing the stoichiometric coefficients, which quantify the ratio of reactants to products, helps in finding the exact numbers needed to balance a reaction.

This process hinges on the balanced chemical equation and the molecular formulae of the compounds involved. It's how we knew that glycerol did not consume the 3 moles of oxygen per mole of compound, as was sought in the original problem. Proper stoichiometric calculation enables us to make precise predictions about the material requirements and the amounts produced in a chemical reaction, which is indispensable in fields like environmental engineering, pharmacology, and materials science.