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Part 2: Mole Calculations 1. How many moles of sodium carbonate are there in 53.6 grams of Na2CO3? 2. How many moles of each atom are there in 33.3 moles of Fe3(PO4)2? 3. How many molecules of dinitrogen tetroxide (N204) are there in 59 g of N204? 4. How many grams does one molecule of carbon monoxide (CO) weigh? 5. How many oxygen gas molecules do you need to make 25 g of water vapor (H₂O)? Balanced chemical equation:

Part 2: Mole Calculations 1. How many moles of sodium carbonate are there in 53.6 grams of Na2CO3? 2. How many moles of each atom are there in 33.3 moles of Fe3(PO4)2? 3. How many molecules of dinitrogen tetroxide (N204) are there in 59 g of N204? 4. How many grams does one molecule of carbon monoxide (CO) weigh? 5. How many oxygen gas molecules do you need to make 25 g of water vapor (H₂O)? Balanced chemical equation:

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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How can we complete part 2? With moles
**Workshop 9: The Mole** The **mole** is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (\(^12\)C isotope). The number of items in 1 mole is called the **Avogadro’s number**: \[ N_A = 6.022141 \times 10^{23} \, \text{1/mol} \] In science, a mole, much like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). Since a mole is just a number, you can have a mole of anything—atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The **molar mass** (or **molar weight**) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole—g/mol. The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought amount of grams of product. **Part 1: Discussion of Mole and Mass** Discuss these questions among your group members: think about water molecules (\(H_2O\)) and sugar molecules (\(C_{12}H_{22}O_{11}\)) and try to predict the answers in the table below. Just predict—do not use a calculator.
Transcribed Image Text:**Workshop 9: The Mole** The **mole** is the unit of measurement for an amount in chemistry and physics. It is defined as the amount of sample that contains as many items as there are atoms in 12 grams of carbon-12 (\(^12\)C isotope). The number of items in 1 mole is called the **Avogadro’s number**: \[ N_A = 6.022141 \times 10^{23} \, \text{1/mol} \] In science, a mole, much like a dozen in our everyday life, allows us to quickly count or compare large (huge!) quantities of items (microscopic objects). Since a mole is just a number, you can have a mole of anything—atoms, molecules, ions, electrons, photons, etc. For any substance, the number of grams in 1 mole is the same as the number of atomic mass units in the molecular weight of the substance. The **molar mass** (or **molar weight**) of a chemical substance is defined as the mass in grams of 1 mole of that substance. The units for molar mass are grams per mole—g/mol. The mole provides a bridge between the atom and the macroscopic amounts of material that we work with in the laboratory or in the industrial setting. For example, it allows chemists to determine how many grams of each of the reactants are needed to produce a sought amount of grams of product. **Part 1: Discussion of Mole and Mass** Discuss these questions among your group members: think about water molecules (\(H_2O\)) and sugar molecules (\(C_{12}H_{22}O_{11}\)) and try to predict the answers in the table below. Just predict—do not use a calculator.
**Part 2: Mole Calculations** 1. How many moles of sodium carbonate are there in 53.6 grams of Na₂CO₃? 2. How many moles of each atom are there in 33.3 moles of Fe₃(PO₄)₂? 3. How many molecules of dinitrogen tetroxide (N₂O₄) are there in 59 g of N₂O₄? 4. How many grams does one molecule of carbon monoxide (CO) weigh? 5. How many oxygen gas molecules do you need to make 25 g of water vapor (H₂O)? Balanced chemical equation: ___________________________________ No graphs or diagrams are present on this page.
Transcribed Image Text:**Part 2: Mole Calculations** 1. How many moles of sodium carbonate are there in 53.6 grams of Na₂CO₃? 2. How many moles of each atom are there in 33.3 moles of Fe₃(PO₄)₂? 3. How many molecules of dinitrogen tetroxide (N₂O₄) are there in 59 g of N₂O₄? 4. How many grams does one molecule of carbon monoxide (CO) weigh? 5. How many oxygen gas molecules do you need to make 25 g of water vapor (H₂O)? Balanced chemical equation: ___________________________________ No graphs or diagrams are present on this page.
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