What is the mass in grams of each of the following samples? (a) 1.505 mol of Ti (b) 0.337 mol of Na (c) 2.583 mol of U

Verified step by step guidance

1. insert step 1: Identify the molar mass of each element from the periodic table.
2. insert step 2: Use the formula: mass (g) = moles × molar mass (g/mol) to calculate the mass for each sample.
3. insert step 3: For (a) 1.505 mol of Ti, multiply the moles by the molar mass of Ti.
4. insert step 4: For (b) 0.337 mol of Na, multiply the moles by the molar mass of Na.
5. insert step 5: For (c) 2.583 mol of U, multiply the moles by the molar mass of U.

Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule or formula unit. For example, the molar mass of titanium (Ti) is approximately 47.87 g/mol, sodium (Na) is about 22.99 g/mol, and uranium (U) is around 238.03 g/mol. Understanding molar mass is essential for converting between moles and grams.

Conversion Between Moles and Grams

To convert moles of a substance to grams, you multiply the number of moles by the substance's molar mass. The formula used is: mass (g) = moles × molar mass (g/mol). This conversion is fundamental in stoichiometry, allowing chemists to relate quantities of reactants and products in chemical reactions. It is crucial for accurately determining the mass of substances in various chemical calculations.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the amounts of reactants and products in a chemical reaction. It is based on the conservation of mass and the mole concept, allowing chemists to predict how much of each substance is needed or produced. Mastery of stoichiometry is vital for solving problems involving chemical reactions, including those requiring mass calculations from moles.