Question

Determine the mass in grams of each of the following. a. 3.57 mol Al b. 42.6 mol S

Short answer

a. Mass (Al) = 96.28 g b. Mass (S) = 1365.56 g

Step-by-step solution

a. Determine the mass in grams of 3.57 mol of Al

First, we need to find the molar mass of aluminum (Al) which is 26.98 g/mol. Next, multiply the given moles (3.57 mol) by the molar mass of Al: Mass = moles × molar mass Mass (Al) = 3.57 mol × 26.98 g/mol Mass (Al) = 96.28 g Hence, the mass of 3.57 mol of aluminum is 96.28 grams.

b. Determine the mass in grams of 42.6 mol of S

First, we need to find the molar mass of sulfur (S) which is 32.06 g/mol. Then, multiply the given moles (42.6 mol) by the sulfur molar mass: Mass = moles × molar mass Mass (S) = 42.6 mol × 32.06 g/mol Mass (S) = 1365.56 g Hence, the mass of 42.6 mol of sulfur is 1365.56 grams.

Key concepts

Moles to Grams Conversion

Converting moles to grams is a fundamental chemical calculation that allows chemists to determine the mass of a substance from the number of moles. This process involves using the molar mass of the substance, which links the amount in moles to the mass in grams. The formula used is simple and straightforward:

• Mass (g) = Moles × Molar Mass (g/mol)

By multiplying the number of moles by the molar mass, you can find the mass of the compound in grams. This calculation is essential in chemical equations where reactions need to happen under specific conditions, ensuring the right amount of product or reactant is used. Understanding this conversion helps with laboratory preparations and theoretical predictions of chemical reactions.

Aluminum Molar Mass

Aluminum (Al) is a commonly used metal known for its lightweight and durable properties. The molar mass of aluminum is 26.98 grams per mole, and this value is used in chemical calculations involving aluminum. When you know the molar mass of aluminum, you can easily convert between moles and grams. For instance, if you have 3.57 moles of aluminum, you can calculate the mass by multiplying by its molar mass: \[ \text{Mass of Al (g)} = 3.57 \text{ mol} \times 26.98 \text{ g/mol} = 96.28 \text{ g} \] Understanding the molar mass of aluminum and how to use it is crucial when working with this element in any chemical context, whether it be studying reactions or working on applications that require specific amounts of aluminum.

Sulfur Molar Mass

Sulfur (S) is a non-metal element essential in many industrial processes and biological systems. It has a molar mass of 32.06 grams per mole. This value is crucial for converting moles of sulfur to grams, often required in stoichiometric calculations. When given moles of sulfur, as in the example of 42.6 moles, you can find the mass using its molar mass: \[ \text{Mass of S (g)} = 42.6 \text{ mol} \times 32.06 \text{ g/mol} = 1365.56 \text{ g} \] Knowing the molar mass allows for accurate measurements and assessments in chemical synthesis and reactions involving sulfur. It helps in determining the right proportions in chemical formulas and aids in laboratory work where precision is key.

Chemical Calculations

Chemical calculations involve various operations necessary for quantifying substances and predicting the outcomes of chemical reactions. They often include conversions and stoichiometric calculations based on balanced equations. Key tools include:

• Understanding moles and molar mass for conversions
• Utilizing balanced chemical equations for proportions
• Applying formulas for volume, pressure, and temperature in gas calculations

Chemical calculations are essential in both academic settings to solve textbook problems and in real-world applications where precise ingredient measures are crucial for safety and efficiency. Mastering these calculations is fundamental for progressing in chemistry and related fields, as they pave the way for accurate analyses and informed decision-making in experiments and industrial applications.