Multiple Choice
The density of the sun is 1.41 g/cm3 and its volume is 1.41 x 1027 m3. How many hydrogen molecules are in the sun if we assume all the mass is hydrogen gas?
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6. Chemical Reactions & Quantities
Mole Concept
2:44 minutesProblem 22e
Textbook Question
Calculate the mass, in grams, for each of the following:
e. 2.08 moles of (NH4)2SO4
Verified step by step guidance1
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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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.
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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.
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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.
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