Domanda del libro di testo
A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. a. Which of the two gases exerts the greater partial pressure?
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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
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Capitolo 5, Problema 79
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g) + 3 F2(g) → 2 ClF3(g) A 2.00-L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 729 mmHg. Identify the limiting reactant. Determine the theoretical yield of ClF3 in grams.
Guida verificata passo dopo passo1
Identify the balanced chemical equation: \( \text{Cl}_2(g) + 3 \text{F}_2(g) \rightarrow 2 \text{ClF}_3(g) \).
Convert the partial pressures of \( \text{Cl}_2 \) and \( \text{F}_2 \) to moles using the ideal gas law: \( PV = nRT \). Assume \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \) and convert pressures from mmHg to atm.
Determine the mole ratio from the balanced equation and compare the mole ratio of available \( \text{Cl}_2 \) and \( \text{F}_2 \) to find the limiting reactant.
Calculate the moles of \( \text{ClF}_3 \) produced using the stoichiometry of the reaction based on the limiting reactant.
Convert the moles of \( \text{ClF}_3 \) to grams using its molar mass (\( \text{ClF}_3 \) molar mass = 92.45 g/mol).
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Limiting Reactant
The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. To identify the limiting reactant, one must compare the mole ratios of the reactants based on the balanced chemical equation and the initial amounts available. In this case, the stoichiometry of the reaction Cl2 + 3F2 → 2ClF3 will guide the analysis.
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Percorso guidato
01:30
Limiting Reagent Concept
Partial Pressure
Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In this question, the partial pressures of chlorine and fluorine gases are crucial for calculating the number of moles available for the reaction, which is necessary for determining the limiting reactant.
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Percorso guidato
00:48Partial Pressure Calculation
Theoretical Yield
Theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, assuming complete conversion and no losses. It is calculated using the stoichiometry of the balanced equation and the limiting reactant. Once the limiting reactant is identified, the theoretical yield of ClF3 can be determined by converting moles of the limiting reactant to grams using its molar mass.
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Percorso guidato
03:09Percent Yield in Reactions
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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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Domanda del libro di testo
Carbon monoxide gas reacts with hydrogen gas to form methanol. CO(g) + 2 H2(g) → CH3OH(g) A 1.50-L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 397 mmHg. Identify the limiting reactant. Determine the theoretical yield of methanol in grams.
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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?
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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
Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. a. Do the atoms in the helium sample have the same average kinetic energy as the atoms in the argon sample?
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