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What is the temperature of 0.52 mol of gas at a pressure of 1.3 atm and a volume of 11.8 L?
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Ch.6 - Gases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
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Capitolo 6, Problema 40
What is the pressure in a 15.0-L cylinder filled with 32.7 g of oxygen gas at a temperature of 302 K?
Guida verificata passo dopo passo1
Identify the ideal gas law equation: \( PV = nRT \).
Calculate the number of moles \( n \) of oxygen gas using its molar mass (\( \text{O}_2 \) has a molar mass of approximately 32.00 g/mol): \( n = \frac{\text{mass}}{\text{molar mass}} \).
Substitute the given values into the ideal gas law equation: \( P = \frac{nRT}{V} \), where \( R \) is the ideal gas constant (0.0821 L·atm/mol·K).
Use the given volume \( V = 15.0 \) L, temperature \( T = 302 \) K, and the calculated moles \( n \) to solve for pressure \( P \).
Perform the calculation to find the pressure \( P \) in atmospheres.
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Ideal Gas Law
The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a 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 one property of a gas if the others are known.
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01:15
Ideal Gas Law Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For oxygen (O2), the molar mass is approximately 32.00 g/mol. Understanding molar mass is essential for converting grams of a substance to moles, which is necessary for using the Ideal Gas Law.
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02:11Molar Mass Concept
Gas Constant (R)
The gas constant (R) is a proportionality constant in the Ideal Gas Law, with a value of 0.0821 L·atm/(K·mol) when pressure is measured in atmospheres and volume in liters. It serves as a bridge between the physical properties of gases and their behavior under various conditions. Knowing the correct value of R is crucial for accurate calculations in gas law problems.
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01:56Gas Constant Values
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An automobile tire has a maximum rating of 38.0 psi (gauge pressure). The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi at a temperature of 12.0 °C. On a hot day, the tire warms to 65.0 °C, and its volume expands to 12.2 L. Does the pressure in the tire exceed its maximum rating? (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.)
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Domanda del libro di testo
What volume is occupied by 12.5 g of argon gas at a pressure of 1.05 atm and a temperature of 322 K? Would the volume be different if the sample were 12.5 g of helium (under identical conditions)?
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Domanda del libro di testo
What volume is occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 305 K?
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What volume is occupied by 0.118 mol of helium gas at a pressure of 0.97 atm and a temperature of 305 K? Would the volume be different if the gas was argon (under the same conditions)?
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A weather balloon is inflated to a volume of 28.5 L at a pressure of 748 mmHg and a temperature of 28.0 °C. The balloon rises in the atmosphere to an altitude of approximately 25,000 ft, where the pressure is 385 mmHg and the temperature is -15.0 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.
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