Domanda del libro di testo
(a) Define the terms limiting reactant and excess reactant.
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
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Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 70
Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 70Capitolo 3, Problema 70
Detonation of nitroglycerin proceeds as follows: 4 C3H5N3O91l2¡ 12 CO21g2 + 6 N21g2 + O21g2 + 10 H2O1g2 (a) If a sample containing 2.00 mL of nitroglycerin 1density = 1.592 g>mL2 is detonated, how many moles of gas are produced?
Guida verificata passo dopo passo1
Calculate the mass of nitroglycerin using its volume and density: \( \text{mass} = \text{volume} \times \text{density} \).
Convert the mass of nitroglycerin to moles using its molar mass: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
Use the balanced chemical equation to determine the mole ratio between nitroglycerin and the total moles of gas produced.
Calculate the total moles of gas produced by multiplying the moles of nitroglycerin by the mole ratio from the balanced equation.
Sum the moles of each gas product (CO2, N2, O2, H2O) to find the total moles of gas produced.
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Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amount of substances consumed and produced in a reaction based on balanced chemical equations. In this case, understanding the stoichiometric coefficients from the balanced equation for nitroglycerin detonation is essential to determine the moles of gas produced.
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Percorso guidato
01:16
Stoichiometry Concept
Molar Mass and Density
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). Density, defined as mass per unit volume, is crucial for converting the volume of a liquid (in this case, nitroglycerin) into mass. By using the density of nitroglycerin, we can find the total mass of the sample, which is necessary for calculating the number of moles of nitroglycerin present before applying stoichiometry.
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02:11Molar Mass Concept
Gas Laws
Gas laws describe the behavior of gases under various conditions of temperature and pressure. In this context, the ideal gas law (PV=nRT) can be applied to relate the number of moles of gas produced to the volume and pressure of the gases generated from the detonation of nitroglycerin. Understanding these principles helps in predicting the behavior of the gaseous products formed during the reaction.
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01:43Combined Gas Law
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The combustion of one mole of liquid octane, CH3(CH2)6CH3, produces 5470 kJ of heat. Calculate how much heat is produced if 1.000 gallon of octane is combusted.
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Domanda del libro di testo
The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g) (b) How many grams of O2 are needed to burn 10.0 g of C8H18?
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Domanda del libro di testo
The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g). (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted? (d) How many grams of CO2 are produced when 15.0 gal of C8H18 are combusted?
Domanda del libro di testo
The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O2 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)?
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