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: Calculate the volume occupied by 35.2 g of methane gas (CH 4) at 25ºC and 1.0 atm. R = 0.08206 L. atm/mol. Ka) 0.0186 Lb) 4.5 Lc) 11.2 Ld) 48.2 Le) 53.7 L

Solution: Calculate the volume occupied by 35.2 g of methane gas (CH 4) at 25ºC and 1.0 atm. R = 0.08206 L. atm/mol. Ka) 0.0186 Lb) 4.5 Lc) 11.2 Ld) 48.2 Le) 53.7 L

Problem

Calculate the volume occupied by 35.2 g of methane gas (CH 4) at 25ºC and 1.0 atm. R = 0.08206 L. atm/mol. K

a) 0.0186 L

b) 4.5 L

c) 11.2 L

d) 48.2 L

e) 53.7 L



Solution

We are asked to find the volume of methane gas (CH4) at the given conditions. Since mass, temperature, and pressure are given, we will use the ideal gas equation to calculate for the volume.

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

In the ideal gas equation, moles are needed but the mass of CH4 is given instead. We’ll calculate the moles of CH4 using its mass and molar mass.

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