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: The following equation shows the combustion of methane.CH4 (g) + 2O2(g) → CO2(g) + 2H2O(g)If 6.0 g of CH4 reacts completely, what is the final pressure of the CO 2 produced and collected in a 1.4 L co

Solution: The following equation shows the combustion of methane.CH4 (g) + 2O2(g) → CO2(g) + 2H2O(g)If 6.0 g of CH4 reacts completely, what is the final pressure of the CO 2 produced and collected in a 1.4 L co

Problem

The following equation shows the combustion of methane.

CH4 (g) + 2O2(g) → CO2(g) + 2H2O(g)

If 6.0 g of CH4 reacts completely, what is the final pressure of the CO 2 produced and collected in a 1.4 L container at a temperature of 21°C?

 

Solution

We are asked to calculate the final pressure of CO2 produced from the combustion of CH4. We can calculate the pressure of the gas using the ideal gas equation:

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, the amount of CO2 in moles is needed but the mass of the CH4 is given instead. We will have to calculate the moles of CO2 produced from CH4 first using the balanced reaction equation and mole to mole comparison.

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