Textbook Question
Consider the apparatus shown in the following drawing. (a) When the valve between the two containers is opened and the gases are allowed to mix, what is the partial pressure of N2 after mixing?
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Ch.10 - Gases
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 10, Problem 60
Acetylene gas, C2H21g2, can be prepared by the reaction ofcalcium carbide with water:CaC21s2 + 2 H2O1l2¡Ca1OH221aq2 + C2H21g2Calculate the volume of C2H2 that is collected over water at23 °C by reaction of 1.524 g of CaC2 if the total pressure ofthe gas is 100.4 kPa. (The vapor pressure of water is tabulatedin Appendix B.)
Verified step by step guidance1
Identify the balanced chemical equation for the reaction: \( \text{CaC}_2 (s) + 2 \text{H}_2\text{O} (l) \rightarrow \text{Ca(OH)}_2 (aq) + \text{C}_2\text{H}_2 (g) \).
Calculate the moles of \( \text{CaC}_2 \) using its molar mass: \( \text{moles of CaC}_2 = \frac{\text{mass of CaC}_2}{\text{molar mass of CaC}_2} \).
Use stoichiometry to find the moles of \( \text{C}_2\text{H}_2 \) produced, knowing that 1 mole of \( \text{CaC}_2 \) produces 1 mole of \( \text{C}_2\text{H}_2 \).
Determine the partial pressure of \( \text{C}_2\text{H}_2 \) by subtracting the vapor pressure of water from the total pressure: \( P_{\text{C}_2\text{H}_2} = P_{\text{total}} - P_{\text{H}_2\text{O}} \).
Use the ideal gas law \( PV = nRT \) to calculate the volume of \( \text{C}_2\text{H}_2 \), where \( P \) is the partial pressure of \( \text{C}_2\text{H}_2 \), \( n \) is the moles of \( \text{C}_2\text{H}_2 \), \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amount of product formed from a given amount of reactant. In this case, understanding the stoichiometric relationship between calcium carbide (CaC2) and acetylene (C2H2) is essential to calculate the volume of gas produced from the mass of CaC2 used.
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Stoichiometry Concept
Gas Laws
Gas laws describe the behavior of gases in relation to pressure, volume, and temperature. The Ideal Gas Law (PV=nRT) is particularly useful for calculating the volume of a gas under specific conditions. In this problem, we need to apply the gas laws to find the volume of acetylene gas produced, taking into account the total pressure and the vapor pressure of water at the given temperature.
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Vapor Pressure of Water
The vapor pressure of water is the pressure exerted by water vapor in equilibrium with its liquid at a given temperature. It is crucial to consider this when collecting gases over water, as the total pressure measured includes both the pressure of the gas and the vapor pressure of water. To find the pressure of the acetylene gas alone, we must subtract the vapor pressure of water from the total pressure.
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Related Practice
Textbook Question
Consider the apparatus shown in the following drawing. (a) When the valve between the two containers is opened and the gases are allowed to mix, how does the volume occupied by the N2 gas change?
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Textbook Question
Magnesium can be used as a 'getter' in evacuated enclosuresto react with the last traces of oxygen. (The magnesium isusually heated by passing an electric current through a wireor ribbon of the metal.) If an enclosure of 5.67 L has a partialpressure of O2 of 7.066 mPa at 30 °C, what mass of magnesiumwill react according to the following equation?2 Mg1s2 + O21g2¡2 MgO1s2
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Textbook Question
Consider a mixture of two gases, A and B, confined in a closed vessel. A quantity of a third gas, C, is added to the same vessel at the same temperature. How does the addition of gas C affect the following: (a) the partial pressure of gas A?
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Textbook Question
During a person's typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume.(a) Calculate the partial pressure of the CO2 in the expiredair at its peak, assuming 1 atm pressure and a body temperature of 37 °C.
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