Textbook Question
Complete the following table for an ideal gas:P V n T101.33 kPa ? L 3.333 mol 300 K
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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 29c
(c) Room temperature is often assumed to be 25 °C. Calculate the molar volume of an ideal gas at 25 °C and 101.3 kPa pressure.
Verified step by step guidance1
Convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T = 25 + 273.15 \).
Use the ideal gas law equation \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Rearrange the ideal gas law to solve for the molar volume \( V_m \), which is the volume per mole: \( V_m = \frac{RT}{P} \).
Substitute the values into the equation: \( R = 8.314 \text{ J/mol·K} \), \( T \) is the temperature in Kelvin from step 1, and \( P = 101.3 \text{ kPa} \).
Calculate the molar volume \( V_m \) using the rearranged equation and the substituted values to find the volume in liters per mole.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of an ideal gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to calculate the behavior of gases under various conditions.
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01:15
Ideal Gas Law Formula
Molar Volume
Molar volume is defined as the volume occupied by one mole of a substance at a given temperature and pressure. For an ideal gas at standard temperature and pressure (0 °C and 101.3 kPa), the molar volume is approximately 22.4 L. However, at different conditions, such as 25 °C and 101.3 kPa, the molar volume can be calculated using the Ideal Gas Law.
Temperature Conversion
In gas calculations, temperature must be expressed in Kelvin rather than Celsius. The conversion from Celsius to Kelvin is done by adding 273.15 to the Celsius temperature. For example, 25 °C is equivalent to 298.15 K. This conversion is crucial for accurately applying the Ideal Gas Law and obtaining correct results.
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02:10Temperature Conversion Example
Related Practice
Textbook Question
Suppose you are given two flasks at the same temperature,one of volume 2 L and the other of volume 3 L. The 2-L flaskcontains 4.8 g of gas, and the gas pressure is x kPa. The 3-Lflask contains 0.36 g of gas, and the gas pressure is 0.1x. Dothe two gases have the same molar mass? If not, which containsthe gas of higher molar mass?
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Textbook Question
(b) What is the molar volume of an ideal gas at STP?
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Textbook Question
(b) If a car tire is filled to a pressure of 220.6 kPa measured at 24 °C, what will be the tire pressure if the tires heat up to 49 °C during driving?
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