Domanda del libro di testo
Lithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2(g) → 2 Li3N(s) What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?
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Ch.5 - Gases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 5, Problema 75
Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 2 NaN3(s) → 2 Na(s) + 3 N2(g) If an automobile air bag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
Guida verificata passo dopo passo1
Identify the balanced chemical equation: \(2 \text{NaN}_3(s) \rightarrow 2 \text{Na}(s) + 3 \text{N}_2(g)\).
Determine the volume of gas produced at STP. At STP, 1 mole of gas occupies 22.4 L. Use this to find the moles of \(\text{N}_2\) needed to fill 11.8 L.
Use the stoichiometry of the reaction to find the moles of \(\text{NaN}_3\) required. From the balanced equation, 2 moles of \(\text{NaN}_3\) produce 3 moles of \(\text{N}_2\).
Calculate the moles of \(\text{NaN}_3\) using the ratio from the balanced equation and the moles of \(\text{N}_2\) calculated in the previous step.
Convert the moles of \(\text{NaN}_3\) to grams using its molar mass (65.01 g/mol).
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Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the quantities of substances involved in a reaction. In this case, the stoichiometric coefficients from the reaction of sodium azide (NaN3) provide the necessary ratios to calculate how much NaN3 is needed to produce a specific volume of nitrogen gas (N2) at standard temperature and pressure (STP).
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Percorso guidato
01:16
Stoichiometry Concept
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. At STP, one mole of an ideal gas occupies 22.4 liters. This law is essential for determining how many moles of nitrogen gas are produced from the decomposition of sodium azide, which can then be used to find the mass of NaN3 required for the airbag to inflate.
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Percorso guidato
01:15Ideal Gas Law Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles. In this problem, knowing the molar mass of sodium azide (NaN3) allows us to calculate how many grams are needed based on the moles derived from the stoichiometric calculations and the Ideal Gas Law.
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Percorso guidato
02:11Molar Mass Concept
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Domanda del libro di testo
Consider the chemical reaction: 2 H2O(l) → 2 H2(g) + O2(g) What mass of H2O is required to form 1.4 L of O2 at a temperature of 315 K and a pressure of 0.957 atm?
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Domanda del libro di testo
CH3OH can be synthesized by the reaction: CO(g) + 2 H2(g) → CH3OH( g) What volume of H2 gas (in L), at 748 mmHg and 86 °C, is required to synthesize 25.8 g CH3OH? How many liters of CO gas, measured under the same conditions, are required?
1778
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1
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Domanda del libro di testo
Ozone is depleted in the stratosphere by chlorine from CF3Cl according to this set of equations:
CF3Cl + UV light → CF3 + Cl
Cl + O3 → ClO + O2
O3 + UV light → O2 + O
ClO + O → Cl + O2
What total volume of ozone at a pressure of 25.0 mmHg and a temperature of 225 K is destroyed when all of the chlorine from 15.0 g of CF3Cl goes through 10 cycles of the given reactions?
1494
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Domanda del libro di testo
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4(g) + H2O(g) → CO(g) + 3 H2(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?
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Domanda del libro di testo
Oxygen gas reacts with powdered aluminum according to the reaction: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) What volume of O2 gas (in L), measured at 782 mmHg and 25 °C, completely reacts with 53.2 g Al?
1567
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