The way of using the coefficients in the balanced overall equation for a reaction to predict with certainty the exponents in the rate law, is to be interpreted. Concept Information: The rate law equation determines the extent to which the product is formed. The rate of a reaction may be defined as the speed at which the chemical reaction proceeds or the concentration of the reactant which transforms into the product, at a particular point in time. The concentrations of the reactants are to be raised to some powers to show their effect on the rate of the reaction . These powers are generalized as the order of the reaction. If the order of any reactant is zero this means that the rate of the reaction is independent on the concentration.
The way of using the coefficients in the balanced overall equation for a reaction to predict with certainty the exponents in the rate law, is to be interpreted. Concept Information: The rate law equation determines the extent to which the product is formed. The rate of a reaction may be defined as the speed at which the chemical reaction proceeds or the concentration of the reactant which transforms into the product, at a particular point in time. The concentrations of the reactants are to be raised to some powers to show their effect on the rate of the reaction . These powers are generalized as the order of the reaction. If the order of any reactant is zero this means that the rate of the reaction is independent on the concentration.
Solution Summary: The author explains how the rate law equation determines the extent to which the product is formed.
Definition Definition Study of the speed of chemical reactions and other factors that affect the rate of reaction. It also extends toward the mechanism involved in the reaction.
Chapter 13, Problem 17RQ
Interpretation Introduction
Interpretation:
The way of using the coefficients in the balanced overall equation for a reaction to predict with certainty the exponents in the rate law, is to be interpreted.
Concept Information:
The rate law equation determines the extent to which the product is formed.
The rate of a reaction may be defined as the speed at which the chemical reaction proceeds or the concentration of the reactant which transforms into the product, at a particular point in time.
The concentrations of the reactants are to be raised to some powers to show their effect on the rate of the reaction. These powers are generalized as the order of the reaction.
If the order of any reactant is zero this means that the rate of the reaction is independent on the concentration.
32. Consider a two-state system in which the low energy level is 300 J mol 1 and the higher energy
level is 800 J mol 1, and the temperature is 300 K. Find the population of each level. Hint: Pay attention
to your units.
A. What is the partition function for this system?
B. What are the populations of each level?
Now instead, consider a system with energy levels of 0 J mol
C. Now what is the partition function?
D. And what are the populations of the two levels?
E. Finally, repeat the second calculation at 500 K.
and 500 J mol 1 at 300 K.
F. What do you notice about the populations as you increase the temperature? At what temperature
would you expect the states to have equal populations?
30. We will derive the forms of the molecular partition functions for atoms and molecules shortly in
class, but the partition function that describes the translational and rotational motion of a homonuclear
diatomic molecule is given by
Itrans (V,T) =
=
2πmkBT
h²
V
grot (T)
4π²IKBT
h²
Where h is Planck's constant and I is molecular moment of inertia.
The overall partition function is qmolec Qtrans qrot.
Find the energy, enthalpy, entropy, and Helmholtz free energy for the translational and rotational
modes of 1 mole of oxygen molecules and 1 mole of iodine molecules at 50 K and at 300 K and with a
volume of 1 m³. Here is some useful data:
Moment of inertia:
I2 I 7.46 x 10-
45
kg m²
2
O2 I 1.91 x 101
-46
kg m²
K
for each reaction step.
Be sure to account for all bond-breaking and bond-making
steps.
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