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: How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)a) 11.6b) 2.32c) 4.64d) 52.0e) 10

Problem

How many moles of O 2 (molar mass = 32.00 g/mol) are needed to react completely with 52.0 L of CH4(g) at STP to produce CO 2 and H2O? (molar mass (CH 4) = 16.04 g/mol)

a) 11.6

b) 2.32

c) 4.64

d) 52.0

e) 104

 

Solution

We will calculate the moles of O2 needed to react with 52.0 L of CH4 using mole to mole comparison.

Let’s first write a balanced reaction equation. We know that the reaction is a combustion reaction since CH4 is made of carbon and hydrogen and is combusted to form carbon dioxide and water as products. 

 Reaction Equation: CH4 + O2 → CO2 + H2O

 C is balanced

 Balance H:               CH4 + O2 → CO2 + 2 H2O

Balance O:               CH4 + 2 O2 → CO2 + 2 H2O

Reactant            Product

C 1                      C  1 
H  4                     H  2 4
O  2 4                  O  3 4

 Balanced reaction Equation: CH4 + 2 O2 → CO2 + 2 H2O

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