Understanding Compound Composition: C6H12O4 Analysis

Introduction to the Compound C6H12O4

The question asks about the composition of the compound with the chemical formula C6H12O4. This formula indicates that each molecule of this compound contains 6 Carbon (C) atoms, 12 Hydrogen (H) atoms, and 4 Oxygen (O) atoms. To understand its composition further, we often look at its molar mass and the mass percentage of each element present.

Calculating the Molar Mass of C6H12O4

The molar mass of a compound is the sum of the atomic masses of all the atoms in its chemical formula. We use the approximate atomic masses for common calculations:

• Carbon (C): 12.011 g/mol (approx. 12 g/mol)
• Hydrogen (H): 1.008 g/mol (approx. 1 g/mol)
• Oxygen (O): 15.999 g/mol (approx. 16 g/mol)

Using the approximate atomic masses, the molar mass of C6H12O4 is calculated as follows:

So, the molar mass of C6H12O4 is approximately 148 g/mol.

Determining Mass Percentage Composition of C6H12O4

The mass percentage of an element in a compound tells us the mass of that element in 100 mass units of the compound. It is calculated using the formula:

Let's calculate the mass percentage for Carbon, Hydrogen, and Oxygen in C6H12O4:

• Mass % of Carbon (C): The total mass of Carbon in one mole of C6H12O4 is \(6 \times 12 = 72\) g. \[ \text{Mass \% of C} = \left( \frac{72 \text{ g}}{148 \text{ g}} \right) \times 100 \approx 48.65\% \]
• Mass % of Hydrogen (H): The total mass of Hydrogen in one mole of C6H12O4 is \(12 \times 1 = 12\) g. \[ \text{Mass \% of H} = \left( \frac{12 \text{ g}}{148 \text{ g}} \right) \times 100 \approx 8.11\% \]
• Mass % of Oxygen (O): The total mass of Oxygen in one mole of C6H12O4 is \(4 \times 16 = 64\) g. \[ \text{Mass \% of O} = \left( \frac{64 \text{ g}}{148 \text{ g}} \right) \times 100 \approx 43.24\% \]

Analyzing the Composition Statements for C6H12O4

Now, let's examine each option provided based on our calculations:

Option 1: 22 atoms per mole

The molecular formula C6H12O4 shows that there are \(6 + 12 + 4 = 22\) atoms in one molecule of C6H12O4. One mole of C6H12O4 contains Avogadro's number of molecules. Therefore, one mole of C6H12O4 contains \(22 \times \text{Avogadro's Number}\) atoms. The statement "22 atoms per mole" is incorrect. It should refer to atoms per molecule or moles of atoms per mole of compound (22 moles of atoms per mole of C6H12O4).

Option 2: twice the mass percent of H as compared to the mass percent of C

Mass % of H \(\approx\) 8.11%. Mass % of C \(\approx\) 48.65%. Twice the mass percent of H is \(2 \times 8.11\% = 16.22\%\). Is 16.22% equal to 48.65%? No. This statement is incorrect.

Option 3: six times the mass percent of C as compared to the mass percent of H

Mass % of C \(\approx\) 48.65%. Mass % of H \(\approx\) 8.11%. Let's check if the mass percent of C is six times the mass percent of H: \(6 \times 8.11\% = 48.66\%\). This value (48.66%) is very close to the calculated mass percent of C (48.65%), with the slight difference due to rounding. A more precise way is to look at the mass ratio within the compound before converting to percentages:

Total mass of C in C6H12O4 = \(6 \times 12 = 72\)

Total mass of H in C6H12O4 = \(12 \times 1 = 12\)

Ratio of total mass of C to total mass of H = \(\frac{72}{12} = 6\).

Since the total mass of carbon in the compound is six times the total mass of hydrogen, the mass percentage of carbon will also be six times the mass percentage of hydrogen. This statement is correct.

Option 4: thrice the mass percent of H as compared to the mass percent of O

Mass % of H \(\approx\) 8.11%. Mass % of O \(\approx\) 43.24%. Thrice the mass percent of H is \(3 \times 8.11\% = 24.33\%\). Is 24.33% equal to 43.24%? No. This statement is incorrect.

Conclusion on C6H12O4 Composition

Based on our detailed analysis of the molar mass and mass percentages, the compound C6H12O4 accurately fits the description that it contains six times the mass percent of C as compared to the mass percent of H.

Revision Table: Chemical Composition Concepts

Additional Information: Importance of Mass Percentage in Chemistry

Mass percentage composition is a fundamental concept in chemistry. It helps in:

• Verifying the purity of a compound.
• Determining the empirical formula of a new compound.
• Calculating the quantities of elements needed to synthesize a specific amount of a compound.
• Comparing the elemental composition of different substances.

Understanding how to calculate and interpret mass percentages provides valuable insight into the quantitative relationships within chemical compounds.