Calculate the mass, in grams, for each of the following:
e. 2.08 moles of (NH₄)₂SO₄

검증된 단계별 안내

Step 1: Write down the formula for the compound, (NH₄)₂SO₄, and identify the molar mass of each element in the compound. The elements are nitrogen (N), hydrogen (H), sulfur (S), and oxygen (O).

Step 2: Calculate the molar mass of (NH₄)₂SO₄ by summing the contributions of each element. Use the periodic table to find the atomic masses: N = 14.01 g/mol, H = 1.008 g/mol, S = 32.07 g/mol, and O = 16.00 g/mol. Multiply these values by the number of atoms of each element in the formula: (2 × N) + (8 × H) + (1 × S) + (4 × O).

Step 3: Add the contributions from all the elements to determine the total molar mass of (NH₄)₂SO₄. This value represents the mass of one mole of the compound in grams.

Step 4: Use the formula for mass: \( \text{Mass (g)} = \text{Moles} \times \text{Molar Mass (g/mol)} \). Substitute the given number of moles (2.08 moles) and the calculated molar mass of (NH₄)₂SO₄ into the equation.

Step 5: Perform the multiplication to find the mass in grams. Ensure that your units cancel appropriately, leaving the final answer in grams.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains approximately 6.022 x 10²³ entities, such as atoms or molecules. Understanding the mole concept is essential for converting between moles and grams, as it provides a bridge between the microscopic scale of atoms and the macroscopic scale of measurable quantities.

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. For example, to find the molar mass of ammonium sulfate, (NH₄)₂SO₄, one must consider the contributions from nitrogen, hydrogen, sulfur, and oxygen in the compound.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It allows chemists to predict how much of a substance is needed or produced in a reaction. In this context, stoichiometry is used to calculate the mass of (NH₄)₂SO₄ from the given number of moles, ensuring accurate conversions and measurements.

Calculate the mass, in grams, for each of the following:e. 2.08 moles of (NH4)2SO4