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: At 20°C (approximately room temperature) the average velocity of N2 molecules in air is 1050 mph. What is the total kinetic energy of 1 mol of N2 molecules moving at this speed?

Solution: At 20°C (approximately room temperature) the average velocity of N2 molecules in air is 1050 mph. What is the total kinetic energy of 1 mol of N2 molecules moving at this speed?

Problem

At 20°C (approximately room temperature) the average velocity of N2 molecules in air is 1050 mph. What is the total kinetic energy of 1 mol of N2 molecules moving at this speed?

Solution

We’re being asked to calculate the kinetic energy of 1 mol of N2 molecules with a speed of 1050 mph. 

To calculate for Kinetic Energy (K.E.), we’re going to use the following equation:

K.E.=12mv2

Ekinetic energy = J
m = mass, in kg
v = velocity of the e- = m/s


We’re going to calculate the Kinetic Energy of N2 molecules using the following steps:

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