CHEM 120 Study Guide - Midterm Guide: High Energy Stereoscopic System, Gibbs Free Energy, Reaction Quotient

52 views3 pages

maroonmallard463

26 Jun 2012

School

Department

Course

Professor

For unlimited access to Study Guides, a Grade+ subscription is required.

cudapuca and 38677 others unlocked

CHEM 120 Full Course Notes

Verified Note

26 documents

Document Summary

Molecules can move (translate), rotate, vibrate, and re-arrange it"s electrons (excite) same as heat. Heat is the net sum of all the motions of molecules. All molecules don"t end up being equal but assume a distribution of these energies. Temperature is not an intrinsic molecular property but an extrinsic one. Conservation of mass: in a system, we neither gain nor lose mass (intuitive, and easy) Conservation of energy: a strange thing called energy" is also conserved. Energy has many different forms, and can interconvert and hide in clever places. Inputs are added together with outputs (isolated systems are easier than open, closed) earth, body, house examples. This work can also be expressed as an expansion against constant (external) pressure: work = force times distance = pextdeltav (in. We can detect the transfer of heat simply as an increase in the temperature of the surroundings.

Related Questions

My first answer was wrong. Can you explain answers?

Qualitative Predictions about Entropy Entropy is the randomness of a system. At the molecular level, entropy can be described in terms of the possible number of different arrangements of particle positions and energies, called microstates. The more microstates the system has, the greater its entropy. Microstates depend on molecular motion. Molecules may undergo three different types of motion: translational motion, vibrational motion, and rotational motion. During translational motion, the entire molecule moves in one direction. During vibrational motion, atoms in a molecule move toward and away from one another. During rotational motion, molecules rotate or spin. The number of molecules, the space available for the molecules, and the energy available to the molecules will impact the number of microstates. Another way of looking at entropy is that the universe is moving toward a broader distribution of energy. The universe has a constant amount of energy as stated in the first law of thermodynamics. The universe started with low entropy (concentrated in the moment before the "big bang") and the entropy has since been constantly increasing by distributing this energy. Heat distribution from high temperature to low temperature is a another example of this phenomenon. Part A Rank these systems in order of decreasing entropy. Rank from highest to lowest entropy. To rank items as equivalent, overlap them. Hints HelpReset Least entropyGreatest entropy 1 mol of neon gas at 273 K and 40 L 1 mol of chlorine gas at 273 K and 40 L 1 mol of hydrogen peroxide gas at 273 K and 40 L 1 mol of neon gas at 273 K and 20 L 1/2 mol of neon gas at 273 K and 20 L 1/2 mol of neon gas at 100 K and 20 L 1/2 mol of liquid neon at 100 K The correct ranking cannot be determined. SubmitMy AnswersGive Up Incorrect; Try Again; 4 attempts r

Please answer and explain!

CHEM 120 Study Guide - Midterm Guide: High Energy Stereoscopic System, Gibbs Free Energy, Reaction Quotient

CHEM 120 Full Course Notes

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 110 Final: Complete and Comprehensive 67 Page Final Exam Study Guide Fall 2015

CHEM 1E03 Lecture Notes - Lecture 7: Heat Capacity, Endothermic Process, Internal Energy

CHEM102 Lecture Notes - State Function, Internal Energy, Horse Length

Related Questions