Question

Two atomic mass units equal how many grams?

Short answer

Two atomic mass units equal approximately \( 3.321078080 \times 10^{-24} \) grams.

Step-by-step solution

Understand the Atomic Mass Unit

An atomic mass unit (amu) is defined as one twelfth of the mass of a carbon-12 atom. This is a standard unit used to express atomic and molecular weights in chemistry.

Know the Conversion Factor

1 atomic mass unit (amu) is equal to \( 1.660539040 \times 10^{-24} \) grams. This conversion factor is essential for translating atomic mass units into grams.

Perform the Calculation

Since two atomic mass units need to be converted to grams, multiply the atomic mass unit value by 2: \[2 \times 1.660539040 \times 10^{-24} = 3.321078080 \times 10^{-24} \text{ grams}\]

State the Result

Conclusively, two atomic mass units are equivalent to approximately \( 3.321078080 \times 10^{-24} \) grams.

Key concepts

Conversion Factor

In chemistry, a conversion factor is a ratio that is used to convert a quantity expressed in one unit into another unit. It essentially bridges the gap between different units of measurement, enabling us to seamlessly switch from one form to another. When discussing atomic mass, the conversion factor between atomic mass units (amu) and grams is crucial to understand.

For instance, to convert from amu to grams, the conversion factor is given as \( 1 ext{ amu} = 1.660539040 \times 10^{-24} \text{ grams} \). This tiny number reflects the incredibly small mass of atoms and molecules. Such conversion allows chemists to work with atomic scale units and connect them to the macroscopic world we measure in grams.

• This factor simplifies the process of making calculations in chemical reactions.
• It provides a bridge between theoretical and practical units.

Understanding this conversion is essential for precise calculations in chemistry.

Atomic and Molecular Weights

Atomic and molecular weights are fundamental concepts in chemistry that describe the mass of atoms and molecules. These masses are typically measured using the atomic mass unit (amu) because it is more convenient for dealing with atom-scale systems.

The atomic weight of an element is the average mass of atoms of that element, measured in amu. It considers the relative abundance of different isotopes. On the other hand, molecular weight refers to the sum of the atomic weights of all atoms in a molecule, also expressed in amu.

• The atomic weight of carbon, for example, is approximately 12 amu.
• These weights allow the comparison and calculation of the masses of different atoms and molecules.

This concept helps chemists predict how substances will interact and allows for precise formulation of chemical equations.

Chemistry Calculation

Chemistry calculations often involve converting units, solving equations, and understanding how quantities relate to each other within a chemical context. The example of converting atomic mass units (amu) to grams is a typical exercise that involves these types of calculations.

To perform such calculations accurately, one must:

• Understand the units involved, both amu and grams.
• Apply the correct conversion factor, which for amu to grams is \(1.660539040 \times 10^{-24}\).
• Ensure calculations account for all components, such as multiplying by the number of units you have (in this case, two).

These steps demonstrate how meticulous and precise one must be in chemistry calculations to ensure accuracy and reliability in scientific work.