Domanda del libro di testo
Consider the reaction: 2 Ag2O(s) → 4 Ag(s) + O2(g) If this reaction produces 15.8 g of Ag(s), what total volume of gas can be collected over water at a temperature of 25 °C and a total pressure of 752 mmHg?
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Ch.6 - Gases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 6, Problema 114a
Consider the reaction:
2 SO2(g) + O2(g) → 2 SO3(g)
a. If 285.5 mL of SO2 reacts with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and the theoretical yield of SO3?
Guida verificata passo dopo passo1
Convert the volumes of SO2 and O2 to moles using the ideal gas law: PV = nRT. Use the given conditions (P = 50.0 mmHg, V = 285.5 mL for SO2 and 158.9 mL for O2, T = 315 K) and R = 62.36 L mmHg/mol K.
Calculate the moles of SO2 using the ideal gas law: n(SO2) = (P * V) / (R * T).
Calculate the moles of O2 using the ideal gas law: n(O2) = (P * V) / (R * T).
Determine the limiting reactant by comparing the mole ratio from the balanced equation (2 SO2 : 1 O2) with the calculated moles of SO2 and O2.
Calculate the theoretical yield of SO3 using the stoichiometry of the balanced equation and the moles of the limiting reactant.
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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. In this case, the reaction of sulfur dioxide (SO2) and oxygen (O2) to form sulfur trioxide (SO3) requires a specific stoichiometric ratio.
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Percorso guidato
01:30
Limiting Reagent Concept
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It involves using mole ratios derived from the coefficients in the balanced equation to determine how much of each reactant is needed or how much product can be formed. In this scenario, stoichiometry will help in calculating the theoretical yield of SO3 from the given volumes of SO2 and O2.
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Percorso guidato
01:16Stoichiometry Concept
Gas Laws
Gas laws describe the behavior of gases in relation to pressure, volume, temperature, and the number of moles. The ideal gas law (PV=nRT) is particularly useful for converting the given volumes of gases at specific conditions into moles, which are necessary for stoichiometric calculations. Understanding how to apply gas laws is essential for determining the amounts of reactants and products in reactions involving gases.
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Percorso guidato
01:43Combined Gas Law
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Domanda del libro di testo
Ammonium nitrate decomposes explosively upon heating according to the balanced equation: 2 NH4NO3(s)¡2 N2( g) + O2( g) + 4 H2O( g) Calculate the total volume of gas (at 125 °C and 748 mmHg) produced by the complete decomposition of 1.55 kg of ammonium nitrate.
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Domanda del libro di testo
Ammonium carbonate decomposes upon heating according to the balanced equation: (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H2O(g) Calculate the total volume of gas produced at 22 °C and 1.02 atm by the complete decomposition of 11.83 g of ammonium carbonate.
7705
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Domanda del libro di testo
Olympic cyclists fill their tires with helium to make them lighter. Calculate the mass of air in an air-filled tire and the mass of helium in a helium-filled tire. Assume that the volume of the tire is 855 mL, that it is filled to a total pressure of 125 psi, and that the temperature is 25 °C. Also, assume an average molar mass for air of 28.8 g/mol. Calculate the mass of air in an air-filled tire.
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