All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: A 0.245-L flask contains 0.467 mol CO2 at 159 °C. Calculate the pressure:(a) using the ideal gas law

Solution: A 0.245-L flask contains 0.467 mol CO2 at 159 °C. Calculate the pressure:(a) using the ideal gas law

Problem

A 0.245-L flask contains 0.467 mol CO2 at 159 °C. Calculate the pressure:

(a) using the ideal gas law

Solution

The ideal gas law is given by:

where P = pressure in atm, V = volume in L, n = moles of gas, R = universal gas constant, and T = temperature in Kelvin.

We can use the ideal gas law to calculate the pressure of the gas. We're given:
V = 0.245 L          T = 159˚C + 273.15 = 432.15 K          n = 0.467 mol

Calculating for the pressure of the gas:

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